Combustion and Burning Fuels: KS3 Chemistry Guide

Combustion is a chemical reaction between a fuel and oxygen that releases energy as heat and light. Every time a gas cooker is lit, a car engine fires, or a candle burns, combustion is taking place. Understanding this reaction — and the difference between complete and incomplete combustion — is a key part of KS3 chemistry, typically taught in Year 8 or Year 9.

What is combustion?

Combustion is an exothermic reaction — it releases energy to the surroundings. Three things must be present for combustion to occur, often remembered as the fire triangle:

Fuel — the substance that burns (e.g. methane, wood, petrol, wax)

Oxygen — must be present in sufficient supply

Heat — enough energy to start the reaction (the ignition temperature)

Remove any one of these three and the fire goes out. This is the principle behind fire extinguishers: a CO₂ extinguisher removes oxygen; a fire blanket removes oxygen; water removes heat.

What is the difference between complete and incomplete combustion?

The amount of oxygen available determines what products form.

Complete combustion

When there is a plentiful supply of oxygen, complete combustion occurs. All the carbon in the fuel is fully oxidised, producing carbon dioxide and water. The flame burns blue and clean (e.g. a Bunsen burner on the air-hole-open setting).

For methane (natural gas), the word equation is:

methane + oxygen → carbon dioxide + water

And the symbol equation:

CH₄ + 2O₂ → CO₂ + 2H₂O

No soot or carbon monoxide is produced. Complete combustion releases the maximum amount of energy from the fuel.

Incomplete combustion

When oxygen supply is limited, incomplete combustion occurs. Carbon is only partially oxidised, producing a mixture of carbon monoxide and soot (unburned carbon particles) alongside carbon dioxide and water. The flame burns yellow or orange and is "smoky" (e.g. a Bunsen burner on the air-hole-closed setting, or a candle).

The possible products of incomplete combustion:

Product | Formula | Hazard
Carbon monoxide | CO | Colourless, odourless, toxic gas — binds to haemoglobin and prevents it carrying oxygen
Soot (carbon) | C | Particulate pollution; stains walls and lungs
Carbon dioxide | CO₂ | Greenhouse gas
Water | H₂O | Harmless

Carbon monoxide is particularly dangerous because it has no colour or smell and cannot be detected by the senses. CO poisoning from faulty boilers or blocked flues causes around 20–30 deaths in England and Wales each year (ONS data). Carbon monoxide alarms are essential in any home with gas appliances.

What are fossil fuels and what do they contain?

Fossil fuels — coal, crude oil, and natural gas — are the remains of ancient organisms that were compressed over millions of years. They are hydrocarbon fuels, meaning they are compounds made primarily of hydrogen and carbon atoms.

Fuel | Main component | State | Main use
Natural gas | Methane (CH₄) | Gas | Heating, cooking, electricity generation
Crude oil (refined) | Various hydrocarbons (e.g. octane C₈H₁₈) | Liquid | Petrol, diesel, aviation fuel, plastics
Coal | Mostly carbon, with some hydrogen | Solid | Electricity generation, steel production

When fossil fuels burn, all the elements they contain react with oxygen. As well as carbon dioxide and water, they produce:

Sulfur dioxide (SO₂) — from sulfur impurities in coal and some oils; dissolves in water to form acid rain (sulfurous acid and sulfuric acid), which damages ecosystems and erodes stone buildings.

Nitrogen oxides (NOₓ) — formed when nitrogen in the air reacts with oxygen at very high temperatures (e.g. in car engines); also contribute to acid rain and photochemical smog.

Environmental impact of burning fuels

Burning fuels has significant environmental consequences:

Climate change — CO₂ is a greenhouse gas that absorbs infrared radiation from Earth's surface and re-emits it, trapping heat in the atmosphere. Since industrialisation, atmospheric CO₂ has risen from around 280 ppm (parts per million) to over 420 ppm in 2024 (NOAA data), driving a rise in average global temperatures.

Acid rain — SO₂ and NOₓ dissolve in rain to form dilute acids (pH 4–5), which damage trees, acidify lakes, and kill aquatic life.

Particulate pollution — fine soot particles from incomplete combustion penetrate deep into the lungs and have been linked to respiratory disease.

Worked example: identifying combustion products

Question: Magnesium burns brightly in air. Is this the same type of reaction as burning methane? What are the products?

Answer:

Both are combustion reactions (reactions with oxygen that release energy as heat and light). However, the products are different:

Methane (CH₄) contains carbon and hydrogen, so its combustion products are CO₂ and H₂O.

Magnesium (Mg) is a metal element containing only magnesium atoms, so it cannot produce CO₂ or H₂O. Instead, it reacts with oxygen to form magnesium oxide (MgO) only:

magnesium + oxygen → magnesium oxide

Magnesium burns with a brilliant white flame. The product is a white powder (magnesium oxide). This is an example of combustion of a metal, not a hydrocarbon.

The Department for Education's Science Programmes of Study for Key Stage 3 requires pupils to understand combustion as an exothermic reaction, the difference between complete and incomplete combustion, the products formed, and the environmental impacts of burning fossil fuels. BBC Bitesize KS3 Chemistry covers combustion, the fire triangle, fossil fuels, and the effects of pollution with diagrams and practice questions.

Frequently asked questions

Why is carbon monoxide so dangerous?

Carbon monoxide (CO) is dangerous because it bonds to haemoglobin in red blood cells far more strongly than oxygen does. Haemoglobin normally picks up oxygen in the lungs and delivers it to cells. When CO binds to haemoglobin, it forms carboxyhaemoglobin, which cannot carry oxygen — so even if you are breathing air that contains plenty of oxygen, your cells become starved of it. Symptoms of CO poisoning include headache, dizziness, and nausea; high concentrations can be fatal. CO is colourless and odourless, so the only protection is a working CO alarm.

What is the fire triangle and why is it useful?

The fire triangle is a model that shows the three things needed for combustion: fuel, oxygen, and heat (ignition). All three must be present simultaneously for a fire to start and continue burning. The model is useful because it shows exactly how to extinguish a fire: remove one side of the triangle. A CO₂ extinguisher floods the area with carbon dioxide, pushing out oxygen. A fire blanket cuts off the oxygen supply. Water cools the fuel below its ignition temperature. In industry and fire safety, this model guides the design of suppression systems.

What is the difference between a fuel and a hydrocarbon?

A fuel is any substance that can be burned to release energy. Fuels include wood, coal, hydrogen gas, and biodiesel. A hydrocarbon is a specific type of molecule made only of hydrogen and carbon atoms. Most fossil fuels are hydrocarbons (methane, octane, etc.), but not all fuels are hydrocarbons — for example, hydrogen gas (H₂) contains no carbon, and wood contains oxygen as well as carbon and hydrogen. When a hydrocarbon burns completely, the products are always carbon dioxide and water. When a non-hydrocarbon fuel burns, the products depend on what elements it contains.

Why does incomplete combustion produce a yellow flame?

The yellow colour of a candle flame or a Bunsen with the air hole closed comes from tiny glowing soot particles (carbon). When there is insufficient oxygen to convert all the carbon to CO₂, some carbon atoms clump together into soot particles. These particles are heated by the reaction to incandescence — they glow yellow-orange, the same way a hot metal glows. When oxygen is plentiful (blue flame), there are no soot particles left to glow, and the faint blue colour comes from excited molecules of CH and C₂ in the reaction zone.

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