Your browser is not supported

Sorry but it looks as if your browser is out of date. To get the best experience using our site we recommend that you upgrade or switch browsers.

Find a solution

  • Skip to main content
  • Skip to navigation

chemistry assignment on fuels

  • Back to parent navigation item
  • Primary teacher
  • Secondary/FE teacher
  • Early career or student teacher
  • Higher education
  • Curriculum support
  • Literacy in science teaching
  • Periodic table
  • Interactive periodic table
  • Climate change and sustainability
  • Resources shop
  • Collections
  • Post-lockdown teaching support
  • Remote teaching support
  • Starters for ten
  • Screen experiments
  • Assessment for learning
  • Microscale chemistry
  • Faces of chemistry
  • Classic chemistry experiments
  • Nuffield practical collection
  • Anecdotes for chemistry teachers
  • On this day in chemistry
  • Global experiments
  • PhET interactive simulations
  • Chemistry vignettes
  • Context and problem based learning
  • Journal of the month
  • Chemistry and art
  • Art analysis
  • Pigments and colours
  • Ancient art: today's technology
  • Psychology and art theory
  • Art and archaeology
  • Artists as chemists
  • The physics of restoration and conservation
  • Ancient Egyptian art
  • Ancient Greek art
  • Ancient Roman art
  • Classic chemistry demonstrations
  • In search of solutions
  • In search of more solutions
  • Creative problem-solving in chemistry
  • Solar spark
  • Chemistry for non-specialists
  • Health and safety in higher education
  • Analytical chemistry introductions
  • Exhibition chemistry
  • Introductory maths for higher education
  • Commercial skills for chemists
  • Kitchen chemistry
  • Journals how to guides
  • Chemistry in health
  • Chemistry in sport
  • Chemistry in your cupboard
  • Chocolate chemistry
  • Adnoddau addysgu cemeg Cymraeg
  • The chemistry of fireworks
  • Festive chemistry
  • Education in Chemistry
  • Teach Chemistry
  • On-demand online
  • Live online
  • Selected PD articles
  • PD for primary teachers
  • PD for secondary teachers
  • What we offer
  • Chartered Science Teacher (CSciTeach)
  • Teacher mentoring
  • UK Chemistry Olympiad
  • Who can enter?
  • How does it work?
  • Resources and past papers
  • Top of the Bench
  • Schools' Analyst
  • Regional support
  • Education coordinators
  • RSC Yusuf Hamied Inspirational Science Programme
  • RSC Education News
  • Supporting teacher training
  • Interest groups

A primary school child raises their hand in a classroom

  • More from navigation items

Organic chemistry worksheets | 14–16 years

  • 1 Introduction
  • 2 Crude oil
  • 3 Hydrocarbons
  • 4 Cracking hydrocarbons
  • 7 Carboxylic acids
  • 8 Addition polymerisation
  • 9 Condensation polymerisation
  • 10 Natural polymers
  • 11 Burning hydrocarbons
  • 12 Reactions of alkanes and alcohols

Hydrocarbons

By Rob King

  • Five out of five
  • No comments

Differentiated, editable worksheets providing a wide range of assessment questions exploring hydrocarbons, including structural formulae, writing word equations and balancing symbol equations

In context worksheets

These write-on worksheets will ask learners to use their knowledge of hydrocarbons in an applied context. Calculation questions are included to give opportunities to practise mathematical skills within this topic. Foundation and higher level worksheets are available and fully editable versions give you the flexibility to select the questions most relevant to a particular lesson. The teacher versions (also editable) give answers to all questions.

Foundation level

  • Download the student worksheet as MS Word or pdf .
  • Download the teacher version including answers to all questions as MS Word or pdf .

Higher level

Knowledge check worksheets.

Provide a series of questions on hydrocarbons to assess learners’ knowledge and understanding of this topic at both foundation and higher levels. The worksheets could be used for individual student work in class or at home. Separate answer sheets allow these resources to be used by teachers or by students during self-assessment of progress.

  • Download the student worksheet as  MS Word  or  pdf .
  • Download the teacher version including answers to all questions as  MS Word  or  pdf .
  • Download the teacher version including answers to all questions as  MS Word  or  pdf .

In context sheet - Hydrocarbons - Foundation - Student

In context sheet - hydrocarbons - foundation - teacher, in context sheet - hydrocarbons - higher - student, in context sheet - hydrocarbons - higher - teacher, knowledge check worksheet - hydrocarbons - foundation - student, knowledge check worksheet - hydrocarbons - foundation - teacher, knowledge check worksheet - hydrocarbons - higher - student, knowledge check worksheet - hydrocarbons - higher - teacher.

Bio-Bug bridge GENeco image

Introduction

Person putting petrol into a car

Cracking hydrocarbons

Fresh assorted fruits and berries

Carboxylic acids

ice-hockey-sport-players-P95UQBE

Addition polymerisation

Polyester fabric clothing label with laundry instructions

Condensation polymerisation

Organic fruit and vegetables and superfoods

Natural polymers

Car engine emitting nitrogen dioxide

Burning hydrocarbons

Ethanol molecular model

Reactions of alkanes and alcohols

  • 14-16 years
  • Maths skills
  • Organic chemistry

Specification

  • Standard temperature and pressure (s.t.p). Molar volume ar s.t.p., molar mass, relative molar mass (Mr).
  • Alkanes, alkenes and alkynes as homologous series. For alkynes only ethyne to be considered.
  • Systematic names, stuctural formulas and structural isomers of alkanes to C-5.
  • Chemical reactions can result in a change in temperature. Exothermic and endothermic reactions (and changes of state).
  • Combustion of alkanes and other hydrocarbons.
  • Recognise and use significant figures as appropriate.
  • Use of alkanes as as fuels.
  • Awareness of the contributions of chemistry to society, e.g. provision of pure water, fuels, metals, medicines, detergents, enzymes, dyes, paints, semiconductors, liquid crystals and alternative materials, such as plastics, and synthetic fibres; increasi…
  • Equations (full and ionic).
  • The melting and boiling points of molecular substances are influenced by the strength of these intermolecular forces.
  • Alkanes are used as fuels.
  • Alkanes are saturated hydrocarbons.
  • 6. be able to write balanced full and ionic equations, including state symbols, for chemical reactions
  • 8. know the general formula for alkanes
  • 9. know that alkanes and cycloalkanes are saturated hydrocarbons
  • 1. know that a hydrocarbon is a compound of hydrogen and carbon only
  • 20 i. understand, in terms of intermolecular forces, physical properties shown by materials, including: the trends in boiling temperatures of alkanes with increasing chain length
  • Chemical reactions can be represented by word equations or equations using symbols and formulae.
  • Write formulae and balanced chemical equations for the reactions in this specification.
  • Chemical equations can be interpreted in terms of moles.
  • Some properties of hydrocarbons depend on the size of their molecules, including boiling point, viscosity and flammability. These properties influence how hydrocarbons are used as fuels.
  • Students should be able to recall how boiling point, viscosity and flammability change with increasing molecular size.
  • The combustion of hydrocarbon fuels releases energy. During combustion, the carbon and hydrogen in the fuels are oxidised. The complete combustion of a hydrocarbon produces carbon dioxide and water.
  • Students should be able to write balanced equations for the complete combustion of hydrocarbons with a given formula.
  • Crude oil is a mixture of a very large number of compounds. Most of the compounds in crude oil are hydrocarbons, which are molecules made up of hydrogen and carbon atoms only.
  • Most of the hydrocarbons in crude oil are hydrocarbons called alkanes. The general formula for the homologous series of alkanes is C₂H₂ₙ₊₂
  • The first four members of the alkanes are methane, ethane, propane and butane.
  • Alkane molecules can be represented in the following forms: (C₂H₆ or drawn out version). Students should be able to recognise substances as alkanes given their formulae in these forms.
  • Describe the fractions as largely a mixture of compounds of formula CₙH₂ₙ₊₂ which are members of the alkane homologous series.
  • Most of the hydrocarbons in crude oil are hydrocarbons called alkanes. The general formula for the homologous series of alkanes is CₙH₂ₙ₊₂
  • 0.3 Write balanced chemical equations, including the use of the state symbols (s), (l), (g) and (aq)
  • 8.1 Recall that hydrocarbons are compounds that contain carbon and hydrogen only
  • 8.4 Recall the names and uses of the following fractions: gases, used in domestic heating and cooking; petrol, used as fuel for cars, kerosene, used as fuel for aircraft; diesel oil, used as fuel for some cars and trains; fuel oil, used as fuel for large…
  • 8.5 Explain how hydrocarbons in different fractions differ from each other in: the number of carbon and hydrogen atoms their molecules contain; boiling points; ease of ignition; viscosity; and are mostly members of the alkane homologous series
  • 8.6 Explain an homologous series as a series of compounds which: have the same general formula; differ by CH₂ in molecular formulae from neighbouring compounds; show a gradual variation in physical properties, as exemplified by their boiling points; have…
  • 8.7 Describe the complete combustion of hydrocarbon fuels as a reaction in which: carbon dioxide and water are produced; energy is given out
  • 9.10C Recall the formulae of molecules of the alkanes, methane, ethane, propane and butane, and draw the structures of these molecules, showing all covalent bonds
  • 9.11C Explain why the alkanes are saturated hydrocarbons
  • 9.16C Describe how the complete combustion of alkanes and alkenes involves the oxidation of the hydrocarbons to produce carbon dioxide and water
  • 8.2 Describe crude oil as: a complex mixture of hydrocarbons; containing molecules in which carbon atoms are in chains or rings (names, formulae and structures of specific ring molecules not required); an important source of useful substances…
  • C3.4.1 recall that crude oil is a main source of hydrocarbons and is a feedstock for the petrochemical industry
  • C3.4.4 describe the fractions of crude oil as largely a mixture of compounds of formula CₙH₂ₙ₊₂ which are members of the alkane homologous series
  • C3.4.17 name and draw the structural formulae, using fully displayed formulae, of the first four members of the straight chain alkanes and alkenes, alcohols and carboxylic acids
  • C3.4.18 predict the formulae and structures of products of reactions (combustion, addition across a double bond and oxidation of alcohols to carboxylic acids) of the first four and other given members of these homologous series
  • C6.1j describe the fractions as largely a mixture of compounds of formula CₙH₂ₙ₊₂ which are members of the alkane homologous series
  • C6.1k recall that crude oil is a main source of hydrocarbons and is a feedstock for the petrochemical industry
  • C6.2b name and draw the structural formulae, using fully displayed formulae, of the first four members of the straight chain alkanes, alkenes, alcohols and carboxylic acids
  • C6.2c predict the formulae and structures of products of reactions of the first four and other given members of the homologous series of alkanes, alkenes and alcohols
  • C6.2l describe the fractions as largely a mixture of compounds of formula CₙH₂ₙ₊₂ which are members of the alkane homologous series
  • Alkanes: are a homologous series of saturated hydrocarbons
  • can be represented by the general formula CₙH₂ₙ₊₂
  • Straight-chain and branched alkanes can be systematically named from structural formulae containing no more than 8 carbons in the longest chain.
  • Molecular formulae can be written and structural formulae can be drawn, from the systematic names of straight-chain and branched alkanes, containing no more than 8 carbons in the longest chain.
  • A homologous series is a family of compounds with the same general formula and similar chemical properties.
  • Patterns are often seen in the physical properties of the members of a homologous series.
  • The subsequent members of a homologous series show a general increase in their melting and boiling points. This pattern is attributed to increasing strength of the intermolecular forces as the molecular size increases. The type of intermolecular force do…
  • Hydrocarbons are compounds containing only hydrogen and carbon atoms.
  • Compounds containing only single carbon–carbon bonds are described as saturated.
  • Compounds containing at least one carbon–carbon double bond are described as unsaturated.
  • The structure of any molecule can be drawn as a full or a shortened structural formula.
  • (f) the combustion reactions of hydrocarbons and other fuels
  • (k) the general formula CₙH₂ₙ₊₂ for alkanes and CₙH₂ₙ for alkenes
  • (l) the names and molecular and structural formulae for simple alkanes and alkenes
  • (n) the names of more complex alkanes and alkenes
  • 2.5.2 define a homologous series as a family of organic molecules that have the same general formula, show similar chemical properties, show a gradation in their physical properties and differ by a CH₂ group;
  • 2.5.3 recall that a hydrocarbon is a compound/molecule consisting of hydrogen and carbon only;
  • 2.5.4 recall the general formula of the alkanes and the molecular formula, structural formula and state at room temperature and pressure of methane, ethane, propane and butane;
  • 2.5.9 describe the complete combustion of alkanes to produce carbon dioxide and water, including observations and tests to identify the products.
  • 1.7.6 calculate the reacting masses of reactants or products, given a balanced symbol equation and using moles and simple ratio, including examples here there is a limiting reactant;
  • 1.7.5 calculate the reacting masses of reactants or products, given a balanced symbol equation and using moles and simple ratio, including examples here there is a limiting reactant;

Related articles

Paracetamol background information cover image

Paracetamol book | Background information

Explore the key elements of paracetamol, and lay a strong foundation of background information.

Paracetamol presentation cover image

Paracetamol book | Presentation activity

Learners put their audio and visual skills to use, on the topic of paracetamol, with this guide on creating a compelling presentation

Paracetamol book | The extraction and purification of paracetamol from tablets

How pure is paracetamol? This practical lets learners distil and tablets and answer that very question.

No comments yet

Only registered users can comment on this article., more from resources.

q2

Paracetamol book | The formation of an amide

Explore the formation of an amide with this practical experiment suitable for learners ages 16-18

The preparation of paracetamol cover image

Paracetamol book | The preparation of paracetamol

 The first of three steps, in practical experiments, that show learners how to prepare paracetamol

The quantitative analysis of various formulations of paracetamol cover image

Paracetamol book | The quantitative analysis of various formulations of paracetamol

An experiment to show learners to analyse several different formulations of paracetamol and create and quantitative judgment of them.

  • Contributors
  • Email alerts

Site powered by Webvision Cloud

swayam-logo

Fundamentals of Combustion

Note: This exam date is subjected to change based on seat availability. You can check final exam date on your hall ticket.

Page Visits

Course layout, books and references, instructor bio.

chemistry assignment on fuels

Prof. V. Raghavan

Course certificate.

chemistry assignment on fuels

DOWNLOAD APP

chemistry assignment on fuels

SWAYAM SUPPORT

Please choose the SWAYAM National Coordinator for support. * :

  • Chemistry Articles

A fuel cell can be defined as an electrochemical cell that generates electrical energy from fuel via an electrochemical reaction.

Table of Content

  • Fuel Cell Definition

Working of Fuel Cell

Types of fuel cells.

  • Applications of Fuel Cells

What is a Fuel Cell?

Fuel cells require a continuous input of fuel and an oxidizing agent (generally oxygen) in order to sustain the reactions that generate the electricity. Therefore, these cells can constantly generate electricity until the supply of fuel and oxygen is cut off.

Despite being invented in the year 1838, fuel cells began commercial use only a century later when they were used by NASA to power space capsules and satellites. Today, these devices are used as the primary or secondary source of power for many facilities including industries, commercial buildings, and residential buildings.

A fuel cell is similar to  electrochemical cells , which consists of a cathode, an anode, and an electrolyte. In these cells, the electrolyte enables the movement of the protons.

Recommended Videos

chemistry assignment on fuels

The reaction between hydrogen and oxygen can be used to generate electricity via a fuel cell. Such a cell was used in the Apollo space programme and it served two different purposes – It was used as a fuel source as well as a source of drinking water (the water vapour produced from the cell, when condensed, was fit for human consumption).

The working of this fuel cell involved the passing of hydrogen and oxygen into a concentrated solution of sodium hydroxide via carbon electrodes. The cell reaction can be written as follows:

Cathode Reaction: O 2 + 2H 2 O + 4e – → 4OH –

Anode Reaction: 2H 2 + 4OH – → 4H 2 O + 4e –

Net Cell Reaction: 2H 2 + O 2 → 2H 2 O

However, the reaction rate of this electrochemical reaction is quite low. This issue is overcome with the help of a catalyst such as platinum or palladium. In order to increase the effective surface area, the catalyst is finely divided before being incorporated into the electrodes.

A block diagram of this fuel cell is provided below.

Fuel Cell Block Diagram

The efficiency of the fuel cell described above in the generation of electricity generally approximates to 70% whereas thermal power plants have an efficiency of 40%. This substantial difference in efficiency is because the generation of electric current in a thermal power plant involves the conversion of water into steam, and the usage of this steam to rotate a turbine. Fuel cells, however, offer a platform for the direct conversion of chemical energy into electrical energy.

Despite working similarly, there exist many varieties of fuel cells. Some of these types of fuel cells are discussed in this subsection.

The Polymer Electrolyte Membrane (PEM) Fuel Cell

  • These cells are also known as proton exchange membrane fuel cells (or PEMFCs).
  • The temperature range that these cells operate in is between 50 o C to 100 o C
  • The electrolyte used in PEMFCs is a polymer which has the ability to conduct protons.
  • A typical PEM fuel cell consists of bipolar plates, a catalyst, electrodes, and the polymer membrane.
  • Despite having eco-friendly applications in transportation, PEMFCs can also be used for the stationary and portable generation of power.

Phosphoric Acid Fuel Cell

  • These fuel cells involve the use of phosphoric acid as an electrolyte in order to channel the H +
  • The working temperatures of these cells lie in the range of 150 o C – 200 o C
  • Electrons are forced to travel to the cathode via an external circuit because of the non-conductive nature of phosphoric acid .
  • Due to the acidic nature of the electrolyte, the components of these cells tend to corrode or oxidize over time.

Solid Acid Fuel Cell

  • A solid acid material is used as the electrolyte in these fuel cells.
  • The molecular structures of these solid acids are ordered at low temperatures.
  • At higher temperatures, a phase transition can occur which leads to a huge increase in conductivity.
  • Examples of solid acids include CsHSO 4 and CsH 2 PO 4 ( cesium hydrogen sulfate and cesium dihydrogen phosphate respectively)

Alkaline Fuel Cell

  • This was the fuel cell which was used as the primary source of electricity in the Apollo space program.
  • In these cells, an aqueous alkaline solution is used to saturate a porous matrix, which is in turn used to separate the electrodes .
  • The operating temperatures of these cells are quite low (approximately 90 o C).
  • These cells are highly efficient. They also produce heat and water along with electricity.

Solid Oxide Fuel Cell

  • These cells involve the use of a solid oxide or a ceramic electrolyte (such as yttria-stabilized zirconia).
  • These fuel cells are highly efficient and have a relatively low cost (theoretical efficiency can even approach 85%).
  • The operating temperatures of these cells are very high (lower limit of 600 o C, standard operating temperatures lie between 800 and 1000 o C).
  • Solid oxide fuel cells are limited to stationary applications due to their high operating temperatures.

Molten Carbonate Fuel Cell

  • The electrolyte used in these cells is lithium potassium carbonate salt. This salt becomes liquid at high temperatures, enabling the movement of carbonate ions.
  • Similar to SOFCs, these fuel cells also have a relatively high operating temperature of 650 o C
  • The anode and the cathode of this cell are vulnerable to corrosion due to the high operating temperature and the presence of the carbonate electrolyte.
  • These cells can be powered by carbon-based fuels such as natural gas and biogas.

Applications of fuel cell

Fuel cell technology has a wide range of applications. Currently, heavy research is being conducted in order to manufacture a cost-efficient automobile which is powered by a fuel cell. A few applications of this technology are listed below.

  • Fuel cell electric vehicles, or FCEVs, use clean fuels and are therefore more eco-friendly than internal combustion engine-based vehicles.
  • They have been used to power many space expeditions including the Appolo space program.
  • Generally, the byproducts produced from these cells are heat and water.
  • The portability of some fuel cells is extremely useful in some military applications.
  • These electrochemical cells can also be used to power several electronic devices.
  • Fuel cells are also used as primary or backup sources of electricity in many remote areas.

Frequently Asked Questions – FAQs

What is a fuel cell.

A fuel cell is an electrochemical cell that generates electrical energy from fuel via an electrochemical reaction. It offers high efficiency and zero emissions.

How does a fuel cell differ from conventional methods of energy generation?

A fuel cell is different from the conventional methods of energy generation because, in a fuel cell, chemical energy is directly converted into electrical energy without intermediate conversion into mechanical power.

Why is fuel cell better than the conventional methods of energy generation?

A fuel cell is preferred over conventional methods of energy generation because, in a fuel cell, zero combustion takes place. Thus, carbon dioxide is not produced.

What are the benefits of a fuel cell?

Fuel cells provide clean energy and emit no pollution. Moreover, it also offers high efficiency and zero emissions. No carbon dioxide is produced while generating chemical energy from a fuel cell.

Which electrolyte is used in molten carbonate fuel cells?

Lithium potassium carbonate salt is used as an electrolyte in molten carbonate fuel cells.

Thus, the different types of fuel cells and the working of an alkaline fuel cell are briefly discussed in this article along with some applications of these electrochemical cells. To learn more about this technology and other related topics, register with BYJU’S and download the mobile application on your smartphone.

Quiz Image

Put your understanding of this concept to test by answering a few MCQs. Click ‘Start Quiz’ to begin!

Select the correct answer and click on the “Finish” button Check your score and answers at the end of the quiz

Visit BYJU’S for all Chemistry related queries and study materials

Your result is as below

Request OTP on Voice Call

Leave a Comment Cancel reply

Your Mobile number and Email id will not be published. Required fields are marked *

Post My Comment

chemistry assignment on fuels

  • Share Share

Register with BYJU'S & Download Free PDFs

Register with byju's & watch live videos.

close

Assignment on Chemistry

Chemistry is the branch of science that is concerned with the properties, composition and reactions of various elementary forms of matter. Students those who studies chemistry as a subject are often asked to prepare assignments on chemistry. Researchomatic contains a wide range of chemistry assignments in this section. Theses assignments will assist individuals in preparing their own chemistry assignments.

Molecular mass of alcoholic fuels affect the enthalpy of combustion

  • Click to Read More

Enzyme Action

Cell chemistry, module 2 – case, cellular chemistry, paper chromatography of food dyes, generate free bibliography in all citation styles.

Researchomatic helps you cite your academic research in multiple formats, such as APA, MLA, Harvard, Chicago & Many more. Try it for Free!

chemistry assignment on fuels

Library homepage

  • school Campus Bookshelves
  • menu_book Bookshelves
  • perm_media Learning Objects
  • login Login
  • how_to_reg Request Instructor Account
  • hub Instructor Commons
  • Download Page (PDF)
  • Download Full Book (PDF)
  • Periodic Table
  • Physics Constants
  • Scientific Calculator
  • Reference & Cite
  • Tools expand_more
  • Readability

selected template will load here

This action is not available.

Chemistry LibreTexts

7.9: Fuels as Sources of Energy

  • Last updated
  • Save as PDF
  • Page ID 169709

Learning Objectives

  • To use thermochemical concepts to solve environmental issues.

Our contemporary society requires the constant expenditure of huge amounts of energy to heat our homes, provide telephone and cable service, transport us from one location to another, provide light when it is dark outside, and run the machinery that manufactures material goods. The United States alone consumes almost 10 6 kJ per person per day, which is about 100 times the normal required energy content of the human diet. This figure is about 30% of the world’s total energy usage, although only about 5% of the total population of the world lives in the United States. In contrast, the average energy consumption elsewhere in the world is about 10 5 kJ per person per day, although actual values vary widely depending on a country’s level of industrialization. In this section, we describe various sources of energy and their impact on the environment.

According to the law of conservation of energy, energy can never actually be “consumed”; it can only be changed from one form to another. What is consumed on a huge scale, however, are resources that can be readily converted to a form of energy that is useful for doing work. Energy that is not used to perform work is either stored as potential energy for future use or transferred to the surroundings as heat.

A major reason for the huge consumption of energy by our society is the low efficiency of most machines in transforming stored energy into work. Efficiency can be defined as the ratio of useful work accomplished to energy expended. Automobiles, for example, are only about 20% efficient in converting the energy stored in gasoline to mechanical work; the rest of the energy is released as heat, either emitted in the exhaust or produced by friction in bearings and tires. The production of electricity by coal- or oil-powered steam turbines (Figure \(\PageIndex{1}\)) is can be more than 50% efficient.

9c60f0031161edce4231dfbb04225a80.jpg

In general, it is more efficient to use primary sources of energy directly (such as natural gas or oil) than to transform them to a secondary source such as electricity prior to their use. For example, if a furnace is well maintained, heating a house with natural gas is about 70% efficient. In contrast, burning the natural gas in a remote power plant, converting it to electricity, transmitting it long distances through wires, and heating the house by electric baseboard heaters have an overall efficiency of less than 35%.

The total expenditure of energy in the world each year is about 3 × 10 17 kJ. 80% of this energy is provided by the combustion of fossil fuels: oil, coal, and natural gas (the sources of the energy consumed in the United States in 2019 are shown in Figure \(\PageIndex{2}\)). Natural gas and petroleum are the preferred fuels because many of the products derived from them are gases or liquids that are readily transported, stored, and burned. Natural gas and petroleum are derived from the remains of marine creatures that died hundreds of millions of years ago and were buried beneath layers of sediment. As the sediment turned to rock, the tremendous heat and pressure inside Earth transformed the organic components of the buried sea creatures to petroleum and natural gas.

US Primary Energy Consumption by Energy Source 2019.png

Coal is a complex solid material derived primarily from plants that died and were buried hundreds of millions of years ago and were subsequently subjected to high temperatures and pressures. Because plants contain large amounts of cellulose , derived from linked glucose units, the structure of coal is more complex than that of petroleum (Figure \(\PageIndex{3}\)). In particular, coal contains a large number of oxygen atoms that link parts of the structure together, in addition to the basic framework of carbon–carbon bonds. It is impossible to draw a single structure for coal; however, because of the prevalence of rings of carbon atoms (due to the original high cellulose content), coal is more similar to an aromatic hydrocarbon than an aliphatic one.

imageedit_2_2329899724.jpg

There are four distinct classes of coal (Table \(\PageIndex{1}\)); their hydrogen and oxygen contents depend on the length of time the coal has been buried and the pressures and temperatures to which it has been subjected. Lignite, with a hydrogen:carbon ratio of about 1.0 and a high oxygen content, has the lowest Δ H comb . Anthracite, in contrast, with a hydrogen:carbon ratio of about 0.5 and the lowest oxygen content, has the highest Δ H comb and is the highest grade of coal. The most abundant form in the United States is bituminous coal, which has a high sulfur content because of the presence of small particles of pyrite (FeS 2 ). The combustion of coal releases the sulfur in FeS 2 as SO 2 , which is a major contributor to acid rain. Table \(\PageIndex{2}\) compares the Δ H comb per gram of oil, natural gas, and coal with those of selected organic compounds.

Peat, a precursor to coal, is the partially decayed remains of plants that grow in swampy areas. It is removed from the ground in the form of soggy bricks of mud that will not burn until they have been dried. Even though peat is a smoky, poor-burning fuel that gives off relatively little heat, humans have burned it since ancient times (Figure \(\PageIndex{4}\)). If a peat bog were buried under many layers of sediment for a few million years, the peat could eventually be compressed and heated enough to become lignite, the lowest grade of coal; given enough time and heat, lignite would eventually become anthracite, a much better fuel.

cc6cfe66cff901de905dc5dd1603ed62.jpg

Converting Coal to Gaseous and Liquid Fuels

Oil and natural gas resources are limited. Current estimates suggest that the known reserves of petroleum will be exhausted in about 60 years, and supplies of natural gas are estimated to run out in about 120 years. Coal, on the other hand, is relatively abundant, making up more than 90% of the world’s fossil fuel reserves. As a solid, coal is much more difficult to mine and ship than petroleum (a liquid) or natural gas. Consequently, more than 75% of the coal produced each year is simply burned in power plants to produce electricity. A great deal of current research focuses on developing methods to convert coal to gaseous fuels ( coal gasification) or liquid fuels (coal liquefaction). In the most common approach to coal gasification, coal reacts with steam to produce a mixture of CO and H2 known as synthesis gas, or syngas:Because coal is 70%–90% carbon by mass, it is approximated as C in Equation \(\ref{7.9.1}\).

\[\mathrm{C_{(s)} +H_2O_{(g)} → CO_{(g)}+H_{2(g)}} \;\;\; ΔH= \mathrm{131\: kJ} \label{7.9.1}\]

Converting coal to syngas removes any sulfur present and produces a clean-burning mixture of gases.

Syngas is also used as a reactant to produce methane and methanol. A promising approach is to convert coal directly to methane through a series of reactions:

\(\mathrm{2C(s)+2H_2O(g)→\cancel{2CO(g)}+\cancel{2H_2(g)}}\hspace{20px}ΔH_1= \mathrm{262\: kJ}\\ \mathrm{\cancel{CO(g)}+\cancel{H_2O(g)}→CO_2(g)+\cancel{H_2(g)}}\hspace{20px}ΔH_2=\mathrm{−41\: kJ}\\ \mathrm{\cancel{CO(g)}+\cancel{3H_2(g)}→CH_4(g)+\cancel{H_2O(g)}}\hspace{20px}ΔH_3=\mathrm{−206\: kJ}\\ \overline{\mathrm{Overall:\hspace{10px}2C(s)+2H_2O(g)→CH_4(g)+CO_2(g)}\hspace{20px}ΔH_\ce{comb}= \mathrm{15\: kJ}}\hspace{40px}\label{7.9.2}\)

Burning a small amount of coal or methane provides the energy consumed by these reactions. Unfortunately, methane produced by this process is currently significantly more expensive than natural gas. As supplies of natural gas become depleted, however, this coal-based process may well become competitive in cost.

47a2af05a22627d98b35dce123f0fe15.jpg

Similarly, the techniques available for converting coal to liquid fuels are not yet economically competitive with the production of liquid fuels from petroleum. Current approaches to coal liquefaction use a catalyst to break the complex network structure of coal into more manageable fragments. The products are then treated with hydrogen (from syngas or other sources) under high pressure to produce a liquid more like petroleum. Subsequent distillation, cracking, and reforming can be used to create products similar to those obtained from petroleum. The total yield of liquid fuels is about 5.5 bbl of crude liquid per ton of coal (1 bbl is 42 gal or 160 L). Although the economics of coal liquefaction are currently even less attractive than for coal gasification, liquid fuels based on coal are likely to become economically competitive as supplies of petroleum are consumed.

Example \(\PageIndex{1}\)

If bituminous coal is converted to methane by the process in Equation \(\ref{7.9.1}\), what is the ratio of the Δ H comb of the methane produced to the enthalpy of the coal consumed to produce the methane? (Note that 1 mol of CH 4 is produced for every 2 mol of carbon in coal.)

Given: chemical reaction and Δ H comb (Table \(\PageIndex{2}\))

Asked for: ratio of Δ H comb of methane produced to coal consumed

A Write a balanced chemical equation for the conversion of coal to methane. Referring to Table \(\PageIndex{2}\), calculate the Δ H comb of methane and carbon.

B Calculate the ratio of the energy released by combustion of the methane to the energy released by combustion of the carbon.

A The balanced chemical equation for the conversion of coal to methane is as follows:

\[\ce{2C (s) + 2H2O(g) → CH4(g) + CO2(g)} \nonumber\]

Thus 1 mol of methane is produced for every 2 mol of carbon consumed. The Δ H comb of 1 mol of methane is

The Δ H comb of 2 mol of carbon (as coal) is

B The ratio of the energy released from the combustion of methane to the energy released from the combustion of carbon is

The energy released from the combustion of the product (methane) is 131% of that of the reactant (coal). The fuel value of coal is actually increased by the process!

How is this possible when the law of conservation of energy states that energy cannot be created? The reaction consumes 2 mol of water (\(ΔH^\circ_\ce{f}=\mathrm{−285.8\: kJ/mol}\)) but produces only 1 mol of CO2 (\(ΔH^\circ_\ce{f}=\mathrm{−393.5\: kJ/mol}\)). Part of the difference in potential energy between the two (approximately 180 kJ/mol) is stored in CH4 and can be released during combustion.

Exercise \(\PageIndex{1}\)

Using the data in Table \(\PageIndex{2}\), calculate the mass of hydrogen necessary to provide as much energy during combustion as 1 bbl of crude oil (density approximately 0.75 g/mL).

The Carbon Cycle and the Greenhouse Effect

Even if carbon-based fuels could be burned with 100% efficiency, producing only CO 2 (g) and H 2 O(g), doing so could still potentially damage the environment when carried out on the vast scale required by an industrial society. The amount of CO 2 released is so large and is increasing so rapidly that it is apparently overwhelming the natural ability of the planet to remove CO 2 from the atmosphere. In turn, the elevated levels of CO 2 are thought to be affecting the temperature of the planet through a mechanism known as the greenhouse effect. As you will see, there is little doubt that atmospheric CO 2 levels are increasing, and the major reason for this increase is the combustion of fossil fuels. There is substantially less agreement, however, on whether the increased CO 2 levels are responsible for a significant increase in temperature.

The Global Carbon Cycle

Figure \(\PageIndex{5}\) illustrates the global carbon cycle, the distribution and flow of carbon on Earth. Normally, the fate of atmospheric CO 2 is to either (1) dissolve in the oceans and eventually precipitate as carbonate rocks or (2) be taken up by plants. The rate of uptake of CO 2 by the ocean is limited by its surface area and the rate at which gases dissolve, which are approximately constant. The rate of uptake of CO 2 by plants, representing about 60 billion metric tons of carbon per year, partly depends on how much of Earth’s surface is covered by vegetation. Unfortunately, the rapid deforestation for agriculture is reducing the overall amount of vegetation, and about 60 billion metric tons of carbon are released annually as CO 2 from animal respiration and plant decay. The amount of carbon released as CO 2 every year by fossil fuel combustion is estimated to be about 5.5 billion metric tons. The net result is a system that is slightly out of balance, experiencing a slow but steady increase in atmospheric CO 2 levels (Figure \(\PageIndex{6}\)). As a result, average CO 2 levels have increased by about 30% since 1850.

7512770d9c759f8934f7dde0f292ed93.jpg

Most of Earth’s carbon is found in the crust, where it is stored as calcium and magnesium carbonate in sedimentary rocks. The oceans also contain a large reservoir of carbon, primarily as the bicarbonate ion (HCO 3 − ). Green plants consume about 60 billion metric tons of carbon per year as CO 2 during photosynthesis, and about the same amount of carbon is released as CO 2 annually from animal and plant respiration and decay. The combustion of fossil fuels releases about 5.5 billion metric tons of carbon per year as CO 2 .

28f88ff3861c4b6722425b0bf04b639a.jpg

The Atmospheric Greenhouse Effect

The increasing levels of atmospheric CO 2 are of concern because CO 2 absorbs thermal energy radiated by the Earth, as do other gases such as water vapor, methane, and chlorofluorocarbons. Collectively, these substances are called greenhouse gases; they mimic the effect of a greenhouse by trapping thermal energy in the Earth’s atmosphere, a phenomenon known as the greenhouse effect (Figure \(\PageIndex{7}\)).

8d0689b1b77418332e8eda8064712d6b.jpg

Venus is an example of a planet that has a runaway greenhouse effect. The atmosphere of Venus is about 95 times denser than that of Earth and contains about 95% CO 2 . Because Venus is closer to the sun, it also receives more solar radiation than Earth does. The result of increased solar radiation and high CO 2 levels is an average surface temperature of about 450°C, which is hot enough to melt lead.

Data such as those in Figure Figure \(\PageIndex{6}\) indicate that atmospheric levels of greenhouse gases have increased dramatically over the past 100 years, and it seems clear that the heavy use of fossil fuels by industry is largely responsible. It is not clear, however, how large an increase in temperature ( global warming ) may result from a continued increase in the levels of these gases. Estimates of the effects of doubling the preindustrial levels of CO 2 range from a 0°C to a 4.5°C increase in the average temperature of Earth’s surface, which is currently about 14.4°C. Even small increases, however, could cause major perturbations in our planet’s delicately balanced systems. For example, an increase of 5°C in Earth’s average surface temperature could cause extensive melting of glaciers and the Antarctic ice cap. It has been suggested that the resulting rise in sea levels could flood highly populated coastal areas, such as New York City, Calcutta, Tokyo, Rio de Janeiro, and Sydney. An analysis conducted in 2009 by leading climate researchers from the US National Oceanic and Atmospheric Administration, Switzerland, and France shows that CO 2 in the atmosphere will remain near peak levels far longer than other greenhouse gases, which dissipate more quickly. The study predicts a rise in sea levels of approximately 3 ft by the year 3000, excluding the rise from melting glaciers and polar ice caps. According to the analysis, southwestern North America, the Mediterranean, and southern Africa are projected to face droughts comparable to that of the Dust Bowl of the 1930s as a result of global climate changes.

The increase in CO 2 levels is only one of many trends that can affect Earth’s temperature. In fact, geologic evidence shows that the average temperature of Earth has fluctuated significantly over the past 400,000 years, with a series of glacial periods (during which the temperature was 10°C–15°C lower than it is now and large glaciers covered much of the globe) interspersed with relatively short, warm interglacial periods (Figure \(\PageIndex{8}\)). Although average temperatures appear to have increased by 0.5°C in the last century, the statistical significance of this increase is open to question, as is the existence of a cause-and-effect relationship between the temperature change and CO 2 levels. Despite the lack of incontrovertible scientific evidence, however, many people believe that we should take steps now to limit CO 2 emissions and explore alternative sources of energy, such as solar energy, geothermal energy from volcanic steam, and nuclear energy, to avoid even the possibility of creating major perturbations in Earth’s environment. In 2010, international delegates met in Cancún, Mexico, and agreed on a broad array of measures that would advance climate protection. These included the development of low-carbon technologies, providing a framework to reduce deforestation, and aiding countries in assessing their own vulnerabilities. They avoided, however, contentious issues of assigning emissions reductions commitments.

be8f10e4a8e71d95ba1d95595cde86f6.jpg

Example \(\PageIndex{2}\)

A student at UCLA decided to fly home to New York for Christmas. The round trip was 4500 air miles, and part of the cost of her ticket went to buy the 100 gal of jet fuel necessary to transport her and her baggage. Assuming that jet fuel is primarily n -dodecane (C 12 H 26 ) with a density of 0.75 g/mL, how much energy was expended and how many tons of \(\ce{CO2}\) were emitted into the upper atmosphere to get her home and back?

Given: volume and density of reactant in combustion reaction

Asked for: energy expended and mass of CO 2 emitted

A After writing a balanced chemical equation for the reaction, calculate \(ΔH^\circ_\ce{comb}\)

B Determine the number of moles of dodecane in 100 gal by using the density and molar mass of dodecane and the appropriate conversion factors.

C Obtain the amount of energy expended by multiplying \(ΔH^\circ_\ce{comb}\) by the number of moles of dodecane. Calculate the amount of CO2 emitted in tons by using mole ratios from the balanced chemical equation and the appropriate conversion factors.

A We first need to write a balanced chemical equation for the reaction:

\[\ce{2C12H26 (l) + 37O2(g) -> 24CO2(g) + 26H2O(l)} \nonumber\]

We can calculate \(ΔH^\circ_\ce{comb}\) using the \(ΔH^\circ_\ce{f}\) values corresponding to each substance in the specified phase (phases are not shown for simplicity):

\[\begin{align*} ΔH^\circ_\ce{comb}&=ΣmΔH^\circ_\ce{f}(\ce{products})−ΣnΔH^\circ_\ce{f}(\ce{reactants})\\ &= [24ΔH^\circ_\ce{f}(\ce{CO2}) + 26ΔH^\circ_\ce{f}(\ce{H2O})]−[37ΔH^\circ_\ce{f}(\ce{O2}) + 2ΔH^\circ_\ce{f}(\ce{C12H26})]\\ &= \mathrm{[24(−393.5\: kJ/mol\: CO_2) + 26(−285.8\: kJ/mol\: H_2O)]} \\ &\:\:\:\:\:\mathrm{−[37(0\: kJ/mol\: O_2) + 2(−350.9\: kJ/mol\: C_{12}H_{26})]}\\ &=\mathrm{−16,173.0\: kJ} \end{align*}\]

According to the balanced chemical equation for the reaction, this value is \(ΔH^\circ_\ce{comb}\) for the combustion of 2 mol of n-dodecane. So we must divide by 2 to obtain \(ΔH^\circ_\ce{comb}\) per mole of n-dodecane:

\[ΔH^\circ_\ce{comb}=\mathrm{−8,086.5\; kJ/mol\; C_{12}H_{26}} \nonumber\]

B The number of moles of dodecane in 100 gal can be calculated as follows, using density, molar mass, and appropriate conversion factors:

\(\mathrm{100\: \cancel{gal} \left( \dfrac{3.785 \cancel{L}}{1 \cancel{gal}}\right )\left(\dfrac{1000 \cancel{mL}}{\cancel{L}}\right)\left(\dfrac{0.75 \cancel{g}}{\cancel{mL}}\right)\left(\dfrac{1\: mol}{170.34 \cancel{g}}\right)= 1.7×10^3\: mol\: C_{12}H_{26}}\)

C The total energy released is

\(ΔH^\circ_\ce{comb}= \mathrm{(−8086.5\: kJ/\cancel{mol}) (1.7×10^3 \cancel{mol}) =−1.4×10^7\: kJ}\)

From the balanced chemical equation for the reaction, we see that each mole of dodecane forms 12 mol of \(\ce{CO2}\) upon combustion. Hence the amount of \(\ce{CO2}\) emitted is

\(\mathrm{1.7×10^3 \cancel{mol\: C_{12}H_{26}}\left(\dfrac{\dfrac{24}{2} \cancel{mol\: CO_2}}{1 \cancel{mol\: C_{12}H_{26}}}\right)\left(\dfrac{44.0 \cancel{g}}{1 \cancel{mol\: CO_2}}\right)\left(\dfrac{1 \cancel{lb}}{454 \cancel{g}}\right)\left(\dfrac{1\: tn}{2000 \cancel{lb}}\right)= 0.99\: tn}\)

Exercise \(\PageIndex{2}\)

Suppose the student in Example \(\PageIndex{2}\) couldn’t afford the plane fare, so she decided to drive home instead. Assume that the round-trip distance by road was 5572 miles, her fuel consumption averaged 31 mpg, and her fuel was pure isooctane (C 8 H 18 , density = 0.6919 g/mL). How much energy was expended and how many tons of CO 2 were produced during her trip?

2.2 × 10 7 kJ; 1.6 tons of CO 2 (about twice as much as is released by flying)

Thermochemical concepts can be used to calculate the efficiency of various forms of fuel, which can then be applied to environmental issues. More than 80% of the energy used by modern society (about 3 × 10 17 kJ/yr) is from the combustion of fossil fuels. Because of their availability, ease of transport, and facile conversion to convenient fuels, natural gas and petroleum are currently the preferred fuels. Supplies of coal , a complex solid material derived from plants that lived long ago, are much greater, but the difficulty in transporting and burning a solid makes it less attractive as a fuel. Coal releases the smallest amount of energy per gram of any fossil fuel, and natural gas the greatest amount. The combustion of fossil fuels releases large amounts of CO 2 that upset the balance of the carbon cycle and result in a steady increase in atmospheric CO 2 levels. Because CO 2 is a greenhouse gas , which absorbs heat before it can be radiated from Earth into space, CO 2 in the atmosphere can result in increased surface temperatures (the greenhouse effect ). The temperature increases caused by increased CO 2 levels because of human activities are, however, superimposed on much larger variations in Earth’s temperature that have produced phenomena such as the ice ages and are still poorly understood.

chemistry assignment on fuels

Green Chemistry

Selective production of bicyclic alkanes as high-density fuel additives by coupling lignocellulose-derived furanics and phenolics.

High-density fuel addtives are important for heavy transportation. Production of high-density fuel additives from renewable resources receives increasing attention in recent years. Despite progress in the depolymerization of lignin, cellulose, and hemicelluloses, there are limited studies on integrating lignin and carbohydrates to make value-added products. Here we design a route to synthesize high-density fuel additives with lignin-derived monophenolics and carbohydrate-derived furanics. We performed Brønsted base-catalyzed C–C coupling of phenolics and furanics followed by hydrodeoxygenation (HDO) catalyzed by a synthesized Ir-ReOx/SiO2 catalyst. Under an optimized reaction condition, the coupling product of phenolics and furanics, bicyclic furyl phenyl precursors, reached a yield of over 90%, which was further hydrodeoxygenated to bicyclohexyl alkanes with a yield of over 98%. The current two-step strategy demonstrates high-selectivity of preparing high-density hydrocarbon fuels from lignocelluloses and provides a possible way to utilize all components of lignocellulosic biomass in an integrated upgrading pathway.

Supplementary files

  • Supplementary information PDF (1913K)

Article information

Download citation, permissions.

chemistry assignment on fuels

S. Huang, X. Luo, J. Li, S. Liu and L. Shuai, Green Chem. , 2024, Accepted Manuscript , DOI: 10.1039/D4GC00105B

To request permission to reproduce material from this article, please go to the Copyright Clearance Center request page .

If you are an author contributing to an RSC publication, you do not need to request permission provided correct acknowledgement is given.

If you are the author of this article, you do not need to request permission to reproduce figures and diagrams provided correct acknowledgement is given. If you want to reproduce the whole article in a third-party publication (excluding your thesis/dissertation for which permission is not required) please go to the Copyright Clearance Center request page .

Read more about how to correctly acknowledge RSC content .

Social activity

Search articles by author.

This article has not yet been cited.

Advertisements

Fossil Fuel

Fossil fuel is a hydrocarbon deposit, such as petroleum , coal, or natural gas , derived from the accumulated remains of ancient plants and animals and used as fuel. The age of the organisms and their resulting fossil fuels is typically millions of years, and sometimes exceeds 650 million years. Fossil fuels contain high percentages of carbon and include petroleum, coal, and natural gas.

All contain carbon and were formed as a result of geologic processes acting on the remains of organic matter produced by photosynthesis, a process that began in the Archean Eon (4.0 billion to 2.5 billion years ago).

The burning of fossil fuels by humans is the largest source of emissions of carbon dioxide, which is one of the greenhouse gases that allows radiative forcing and contributes to global warming. A small portion of hydrocarbon-based fuels are biofuels derived from atmospheric carbon dioxide, and thus do not increase the net amount of carbon dioxide in the atmosphere.

Fossil fuels are continually being formed via natural processes, they are generally considered to be non-renewable resources because they take millions of years to form and the known viable reserves are being depleted much faster than new ones are being made. Carbon dioxide and other greenhouse gases generated by burning fossil fuels are considered to be one of the principal causes of global warming.

Properties of Fossil Fuel

Fossil fuels are a great source of energy because they originate from living things. The utilization of fossil fuels has enabled large-scale industrial development and largely supplanted water-driven mills, as well as the combustion of wood or peat for heat. Fossil fuels power much of modern civilization; they also see use in fertilizers, plastics and many other chemical compounds. Despite their widely different appearances, coal, natural gas and petroleum oil have several properties in common.

  • Organic Molecules: Without exception, fossil fuels contain organic molecules rings or chains of atoms consisting primarily of carbon. Bituminous coal, natural gas and oil are hydrocarbons, which are combinations chiefly of hydrogen and carbon.
  • Mined Substances: Because they have been trapped underground for millions of years, fossil fuels are extracted by various mining operations such as drilling and digging into the earth. Geologists have identified the rock formations that accompany each type of fuel.
  • Combustible: Fossil fuels are combustible, burning in the presence of oxygen and forming water vapor, carbon dioxide, ash and other byproducts. Their ability to burn comes largely from their carbon content; carbon in the fuel combines with oxygen in the air, giving off large amounts of heat. Components of fossil fuels, such as gasoline, diesel oil and natural gas have different flash points, some burning easily and others taking more energy to ignite.
  • Non-Renewable Fuels: A finite supply of coal, oil and gas exists, making them non-renewable fuels. Although modern prospecting technologies help identify new deposits of fossil fuels, and new methods of extraction make known reserves more productive, these substances form much more slowly than their rates of consumption.

Uses and Advantages of Fossil Fuel

One of the main by-products of fossil fuel combustion is carbon dioxide (CO 2 ). The ever-increasing use of fossil fuels in industry, transportation, and construction has added large amounts of CO 2 to Earth’s atmosphere.

Of the three types of fossil fuels, coal is the only one still in a solid state. It appears as chunks of midnight black rock, which are harvested from the Earth by workers in mining operations. Coal is composed of five different elements: carbon, nitrogen, oxygen, hydrogen, and sulfur. Coal today is used for everything from producing steel and cement to keeping the lights on in homes and businesses.

Natural gas is used primarily to heat homes, power air conditioning systems, and fuel stoves and other cooking appliances. Natural gas is odorless when it is mined from beneath the Earth’s surface, with the smell being added later as a means of alerting people to leaks of the substance.

Oil, also called petroleum, is arguably the most often discussed form of fossil fuel in the world today. A little less than half of the average barrel of oil is refined into gasoline, which is indeed the type of petroleum that we use to fuel our cars. However, other parts of the barrel are refined into oil for asphalt, jet fuel, kerosene, lubricants, and more.

There are many advantages of fossil fuels. Even though they are consumed in mass amounts, they are still abundant and accessible. Fossil fuels provide a large amount of concentrated energy for a relatively low cost. Their abundance allows power plants to be fueled by them, creating a great deal of electricity for the world. Additionally, oil can be transported through the use of pipes, allowing it to be transported relatively easily.

Reference: study.com ,  sciencing.com ,  sciencedaily.com , wikipedia .

Monosaccharide – a most basic form of carbohydrates

Embrittlement – a process of material becoming brittle due to loss of ductility, have you ever wondered how your body converts food into fuel, aeschynite-(nd): occurrence and properties, construction project management, parabola in coordinate geometry, six steps to a scrum transformation, about it help desk software, advantage of an auto billing system, motor cortex, latest post, rural electrification, earthquake engineering – a discipline of engineering, toxins similar to seahorses used to kill insects, the ‘genetic time machine’ uncovers secrets of our dna, scientists identify the most widespread tropical tree species, construction management (cm).

IMAGES

  1. CHEMISTRY ASSIGNMENT SK015 COVER PAGE

    chemistry assignment on fuels

  2. Chemistry 30 Unit 4

    chemistry assignment on fuels

  3. GCSE Edexcel Chemistry Fuels and Earth Science Complete Revision

    chemistry assignment on fuels

  4. The Chemistry of Petrol and Diesel: Infographic

    chemistry assignment on fuels

  5. Fuels 3

    chemistry assignment on fuels

  6. CHEMISTRY 12TH FEBRUARY ASSIGNMENT ANSWERS CGBSE 2021

    chemistry assignment on fuels

VIDEO

  1. Chemistry Lecture Fuel 04

  2. Important questions for semester exam Engineering Chemistry Unit 4 Fuels and Combustion CY3151

  3. Chem 101 Lecture 11: Chapter 5 Gases

  4. Calorific Value of Fuels #shorts #science #chemistry

  5. CH13_Gas Mixtures _part1

  6. Fuels

COMMENTS

  1. 7.9: Fuels as Sources of Energy

    The combustion of fossil fuels releases about 5.5 billion metric tons of carbon per year as CO 2. Figure 7.9.6 7.9. 6: Changes in Atmospheric CO 2 Levels. (a) Average worldwide CO 2 levels have increased by about 30% since 1850.

  2. Chapter 15.7: Fossil Fuels

    The total expenditure of energy in the world each year is about 3 × 10 17 kJ. Today, more than 80% of this energy is provided by the combustion of fossil fuels: oil, coal, and natural gas (The sources of the energy consumed in the United States in 2009 are shown in Figure 15.7.2.) but as Table 15.7.1 from the Wikipedia shows, energy usage is a complex issue.

  3. Crude oil and hydrocarbons

    Edexcel Fuels - Edexcel Crude oil and hydrocarbons Crude oil is a finite resource. Petrol and other fuels are produced from it using fractional distillation and cracking. Combustion products...

  4. Crude oil

    Alkanes are used as fuels. Edexcel Chemistry. Topic 6: Organic Chemistry I. Topic 6B: Alkanes. 8. know the general formula for alkanes; 9. know that alkanes and cycloalkanes are saturated hydrocarbons; 10. understand that alkane fuels are obtained from the fractional distillation, cracking and reforming of crude oil. Reforming is described as ...

  5. (PDF) Fuels and Combustion CHAPTER

    The combustion reaction can be explained as C + O 2 CO 2 + 94 kcals 2H 2 + O 2 2H 2 O + 68.5 kcals The calorific value of a fuel depends mainly on the amount of Carbon and Hydrogen. A good fuel...

  6. Hydrocarbons

    Provide a series of questions on hydrocarbons to assess learners' knowledge and understanding of this topic at both foundation and higher levels. The worksheets could be used for individual student work in class or at home. Separate answer sheets allow these resources to be used by teachers or by students during self-assessment of progress.

  7. Fuels and Fuel Chemistry

    Fuels and fuel chemistry A fuel is any compound that has stored energy. This energy is captured in chemical bonds through processes such as photosynthesis and respiration. Energy is released during oxidation. The most common form of oxidation is the direct reaction of a fuel with oxygen through combustion. Source for information on Fuels and Fuel Chemistry: World of Earth Science dictionary.

  8. 14.1.2 Fuels

    Common Fossil Fuels. A fuel is a substance which when burned, releases heat energy. This heat can be transferred into electricity, which we use in our daily lives. Most common fossil fuels include coal, natural gas and hydrocarbons such as methane and propane which are obtained from crude oil. Hydrocarbons are made from hydrogen and carbon ...

  9. Fuel Chemistry

    The optimal fuel chemistry creates a fuel blend with the highest calorific value expressed as Btu/lb, the lowest moisture, the lowest sulfur and fuel nitrogen expressed in lb/106 Btu (or kJ/kg) sulfur as SO 2 and N, the lowest ash content, also in lb/10 6 Btu, and as high a set of ash fusion temperatures as possible Note that there are eight ...

  10. PDF B.Tech 1st year By

    Introduction A fuel is a substance that contains carbon and hydrogen undergoes combustion in presence of oxygen to gives large amount of energy. Fuel + O2 CO2 + H2O + Energy Classification of Fuel On the basis of occurrence fuel is classified into two categories; natural or primary fuels and artificial or secondary fuels.

  11. Chemistry Assignment

    Engineering Chemistry Assignment No: 01 Fuels Basic Definition: Fuels are any materials that store potential energy in forms that can be practicably released and used for work or as heat energy. The heat energy released by many fuels is converted into mechanical energy via. an engine.

  12. Assignment 1

    Give reason for answer. Explain the determination of calorific value of gaseous fuel using Boy's calorimetric method. A sample of coal was found to have the following composition by mass : C = 75%, H = 5%, O = 12 %, N = 3% and ash = 4%. Calculate Highest and the lowest calorific value of fuel. Guru Gobind Singh Indraprastha University

  13. Types of Fuel

    Chemistry Coal and Petroleum Fuel Types Types Of Fuels What is a fuel? According to the law of conservation of energy: Energy can neither be created nor be destroyed; it can only be changed from one form to another. Thus, we cannot produce energy to do certain work.

  14. Chemistry Assignment

    1. lower boiling points 2. lower viscosity (they flow more easily) 3. Higher flammability (they ignite more easily). OTHER FOSSIL FUELS Crude oil is not the only fossil fuel. Natural gas mainly consists of methane.

  15. Fundamentals of Combustion

    Fundamentals of Combustion. To enable students to apply the knowledge of thermodynamics to combustion. To emphasize the basics of fuels, stoichiometry, chemical kinetics and equilibrium, mass transfer, and different types of combustion process. To explain the mathematics involved in transport processes of a reactive flow, simplifications ...

  16. 8.1.4 Combustion of Fuels

    The combustion of fossil fuels is the major source of atmospheric pollution. Fossil fuels include: coal, oil, natural gas, oil shales and tar sands. Non-renewable fossil fuels are obtained from crude oil by fractional distillation. Petrol is used as a fuel in cars, kerosene is used to fuel aircraft and diesel oil is used as a fuel in some cars ...

  17. Chemistry Assignment 1

    of 9 Department: Mechanical Engineering Applied Chemistry Assignment No. 1 Topic: HCs Fuels Hydrocarbons: - A hydrocarbon is an organic chemical compound composed exclusively of hydrogen and carbon atoms. Hydrocarbons are naturally-occurring compounds and form the basis of crude oil, natural gas, coal, and other important energy sources.

  18. Fuel Cell

    Chemistry Chemistry Articles Fuel Cell Fuel Cell A fuel cell can be defined as an electrochemical cell that generates electrical energy from fuel via an electrochemical reaction. Table of Content Fuel Cell Definition Working of Fuel Cell Types of Fuel Cells Applications of Fuel Cells What is a Fuel Cell?

  19. Engineering Chemistry (TCH-101) Assignment-2 (Topic: Fuels and ...

    of 1 Engineering Chemistry (TCH-101) Assignment-2 (Topic: Fuels and Calorific Value) Q1.In an experiment in a Bomb calorimeter, a solid fuel of 0.90g is burnt. It is observed that increase of temperature is 3.8oC of 4000g of water. The fuel contains 1% of H. calculate

  20. Free Chemistry Assignment & Assignment topics

    Assignment on Chemistry. Chemistry is the branch of science that is concerned with the properties, composition and reactions of various elementary forms of matter. Students those who studies chemistry as a subject are often asked to prepare assignments on chemistry. Researchomatic contains a wide range of chemistry assignments in this section.

  21. 7.9: Fuels as Sources of Energy

    The total yield of liquid fuels is about 5.5 bbl of crude liquid per ton of coal (1 bbl is 42 gal or 160 L). Although the economics of coal liquefaction are currently even less attractive than for coal gasification, liquid fuels based on coal are likely to become economically competitive as supplies of petroleum are consumed.

  22. Selective production of bicyclic alkanes as high-density fuel additives

    High-density fuel addtives are important for heavy transportation. Production of high-density fuel additives from renewable resources receives increasing attention in recent years. Despite progress in the depolymerization of lignin, cellulose, and hemicelluloses, there are limited studies on integrating lign

  23. Fossil Fuel

    Fossil fuel is a hydrocarbon deposit, such as petroleum, coal, or natural gas, derived from the accumulated remains of ancient plants and animals and used as fuel. The age of the organisms and their resulting fossil fuels is typically millions of years, and sometimes exceeds 650 million years. Fossil fuels contain high percentages of carbon and ...