CHEMISTRY: FORM TWO: Topic 4 – FUELS AND ENERGY

Solid fuels include wood, charcoal, peat, lignite, coal, coke, etc. The immediate use of all these fuels is for heating and lighting. However, these fuels have a long history of industrial use. Coal was the fuel for the industrial revolution, from firing furnaces to running steam locomotives and trains. Wood was extensively used to run locomotives. Coal is still used for generation of power until now. For example, in Tanzania the coal mined at Kiwira is used for generation of electricity. Also Tanga Cement Company uses coal as a source of power to run machines for production of cement.

Wood is used as a solid fuel for cooking, heating or, occasionally, as a source of power in steam engines. The use of wood as a fuel source for home heating is as old as civilization itself. Wood fuel is still common throughout much of the world. It is the main source of energy in rural areas.

Wood charcoal yields a large amount of heat in proportion to its quantity than is obtained from a corresponding quantity of wood, and has a further advantage of being smokeless. Wood charcoal is often used for cooking and heating, in blacksmithing, etc.

Animal charcoal is used for sugar refining, water purification, purification of factory air and for removing colouring matter from solutions and from brown sugar. Animal charcoal is made by destructive distillation of animal bones.

Coke is a fuel of great industrial use. Coke is obtained by destructive distillation of coal. Most of the coke produced in industry is used as a reducing agent in the production of metals such as pig iron. A substantial amount of coke is also used for making industrial gases such as water gas and producer gas.

Coke is a better fuel than coal because when it is burning, it produces a clean and smokeless flame. When coal is used as a fuel, it produces many toxic gases during burning. Coke has high heat content and leaves very little ash.

Coal is a complex mixture of substances, and its composition varies from one place to another. It depends on coal’s age and condition under which it was formed. Anthracite is a very hard black coal and it is the oldest of all types of coal.

When coal is heated in a limited supply of air, it decomposes. This thermal decomposition is called destructive distillation of coal. The products are coke, coal tar, ammoniacal liquor and coal gas.

Liquid fuels include petrol (gasoline) diesel, alcohol (spirit), kerosene (paraffin), liquid hydrogen, etc. Liquid fuels have advantage over solid fuels because they produce no solid ashes, and can be regulated by automatic devices. They are relatively more convenient to handle, store and transport than solid fuels.

Most liquid fuels in wide use are derived from fossils. Fossil fuels include coal, natural gas and petroleum. These fuels are formed from remains of sea plants and animals which lived millions of years ago. The remains became buried under layers of sediment. Immense heat and pressure resulted in the formation of coal gas and oil.

Energy produced when petroleum products (diesel, petrol, kerosene, natural gas etc) are burned, originated from the sun. This energy was transferred to animals through their consumption of plants or plant products. When the animals died, got buried, and compressed by heat and pressure, they produced oil which gives off that energy when burnt.

Petroleum fuels are used in cars and in various other machines. Fuels used in cars and lories (petrol and diesel), kerosene (for jet aircraft) and fuel oil (for ships), all came from crude oil. Some oil fuel is also used for electricity generation.

Ethanol burns with a clean, non-smoky flame, giving out quite a lot of heat. On a small scale, ethanol can be used as methylated spirit (ethanol mixed with methanol or other compounds) in spirit lamps and stoves. However, ethanol is such a useful fuel that some countries have developed it as a fuel for cars. In countries where ethanol can be produced cheaply, cars have been adapted to use a mixture of petrol and ethanol as fuel.

Brazil has a climate suitable for growing sugarcane. Ethanol produced by fermentation of sugarcane has been used as an alternative fuel to gasoline (petrol), or mixed with gasoline to produce “gasohol”. Currently, about half of Brazil’s cars run on ethanol or “gasohol”. “Gasohol” now accounts for 10% of the gasoline sales in the U.S.A.

The idea about the use of biofuel for fuelling automobiles and other machines has been borrowed by other countries including Tanzania. However, the programme has raised a bitter concern among different activists. Their doubt is that emphasis on growing crops for biofuel production may take up land that could otherwise be used for growing food crops. This, therefore, would mean that there would not be enough land to grow enough food to feed the ever-increasing human population. Hence, hunger will prevail. Notwithstanding all these shouting, biofuel crop production is there to stay!

The use of gaseous fuels for domestic heating is common in urban areas. Compressed gas that is delivered to our homes in steel cylinders is liquefied propane, butane, or mixture of the two. When the valve is opened, the liquid gas vapourizes quickly into gas and passes through a pipe to the stove. Gaseous fuels are the most convenient fuels to handle, transport and store.

The following is a list of types of gaseous fuels:

• Fuel naturally found in nature: -natural gas -methane from coal mine
• Fuel gas from solid fuels or materials: -gas derived from coal (water gas and producer gas) -gas derived from wastes and biomass (biogas)
• Fuel gas made from petroleum.

Producer gas and water gas are important industrial fuels.

Producer gas

Producer gas is produced by burning a solid carbonaceous fuel, such as coke, in a limited supply of air in a producer furnace. The reaction is exothermic and this makes coke to get hotter. Carbonaceous fuels are fuels that contain a high proportion of carbon. The producer gas is a mixture of carbon monoxide and nitrogen.

When air, mixed with a little steam, is passed through the inlet in the lower part of the furnace, the coke (carbon) combines with oxygen (from air) to form carbon dioxide:

As the carbon dioxide formed rises up through the red-hot coke, it is reduced to carbon monoxide:

Since more heat (406 kJ) is produced in the lower part than is absorbed in the upper part of the furnace (163 kJ), some excess heat is obtained in the long run. This heat keeps the coke hot. The nitrogen gas in the air is not affected at all during the process. Hence, the overall reaction equation may be represented as follows:

As a fuel, producer gas burns to give out carbon dioxide.

Because a good deal of producer gas contains nitrogen, a gas that does not support combustion, it has a lower calorific value compared to water gas. See table 4.2 for comparison.

Water gas

Water gas is produced by passing steam over white-hot coke at 1000°C. The gas is a mixture of hydrogen and carbon monoxide. The reaction is endothermic, causing the coke to cool.

Water gas burns as a fuel to give carbon dioxide and steam.

However, carbon monoxide is a very poisonous gas. The gas made from petroleum or coal contains some carbon monoxide, which makes it poisonous. Natural gas is safer and efficient, as it contains no carbon monoxide.

A good fuel burns easily to produce a large amount of energy. Fuels differ greatly in quality. There are certain characteristics, which make a good fuel. After all, there is no fuel among the different fuels known that posses all the virtues that a good fuel should have. Generally, a good fuel has the following

characteristics:

1. It should be environmentally friendly (not harm the environment) in the course of its production and use, that is, it should not produce harmful or toxic products such as much smoke, carbon dioxide, carbon monoxide, sulphur dioxides, etc, which pollutes the air.
2. It must be affordable to most people i.e. it must be cheap.
3. It should not emit or produce dangerous by-products such as poisonous fumes, vapour or gases.
4. It should have high calorific value i.e. it must burn easily and produce a tremendous quantity of heat energy per unit mass of the fuel.
5. It should be easy and safe to transport, store, handle and use.
6. It should be readily available in large quantities and easily accessible.
7. It should have high pyrometric burning effect (highest temperature that can be reached by a burning fuel). Normally gaseous fuels have the highest pyrometric effect as compared to liquid and solid fuels.
8. It should have a moderate velocity of combustion (the rate at which it burns) to ensure a steady and continuous supply of heat.
9. A good fuel should have an average ignition point (temperature to which the fuel must be heated before it starts burning). A low ignition point is not good because it makes the fuel catch fire easily, which is hazardous, while high ignition point makes it difficult to start a fire with the fuel.
10. A good fuel should have a low content of non-combustible material, which is left as ash or soot when the fuel burns. A high content of no-combustible material tends to lower the heat value of the fuel.

The heating value or calorific value of a substance, usually a fuel or food, is the amount of heat released during the combustion of a specific amount of it. The calorific value is a characteristic of each substance. It is measured in units of energy per unit of substance, usually mass, such as Kcal/Kg, J/g, KJ/Kg, KJ/Mol, MJ/m³, etc. Heating value is commonly determined by use of an instrument called bomb calorimeter.

By custom, the basic calorific value for solid and liquid fuels is the gross calorific value at constant volume, and for gaseous fuels, it is the gross calorific value at constant pressure.

Solid and liquid fuels	Calorific value (MJ/kg)
Alcohols
Ethanol	30
Methanol	23
Coal and coal products
Anthracite (4% water)	36
Coal tar fuels	36 – 41
General purpose coal (5-10% water)	32 – 42
High volatile coking coals (4% water)	35
Low temperature coke (15% water)	26
Medium-volatile coking coal (1% water)	37
Steam coal (1% water)	36
Peat
Peat (20% water)	16
Petroleum and petroleum products
Diesel fuel	46
Gas oil	46
Heavy fuel oil	43
Kerosene	47
Light distillate	48
Light fuel oil	44
Medium fuel oil	43
Petrol	44.80 – 46.9
Wood
Wood (15% water)	16
Gaseous fuels at 15ºC, 101.325 kPa, dry	Calorific value (MJ/m3)
Coal gas coke oven (debenzolized)	20
Coal gas low temperature	34
Commercial butane	118
Commercial propane	94
North sea gas, natural	39
Producer gas coal	6
Producer gas coke	5
Water gas carburetted	19
Water gas blue	11

We burn fuels to provide us with heat energy. The more heat a fuel gives out the better. The amount of heat given out when one mole of fuel burns is called heat of combustion. This is often written as

This value can be measured in the laboratory indirectly by burning the fuel to heat water. Simple apparatus is shown in figure bellow. The basic idea is: Heat gained by the

Heat gained by the water = heat given out by the fuel.

Method

These are the steps:

• Pour a measured volume of water into the tin. Since you know its volume you also know its mass (1 cm³ of water has a mass of 1g).
• Weigh the fuel and its container.
• Measure the temperature of the water.
• Light the fuel and let it burn for a few minutes.
• Measure the water temperature again, to find the increase.
• Reweigh the fuel and container to find how much fuel was burned.

Calculations

It takes 4.2J of energy to raise the temperature of 1g of water by 1ºC. This constant value is called specific heat capacity of water, usually represented as 4.2J_g^-1C^-1 (4.2 joules per gram per centigrade). So, you can calculate the energy given out when the fuel burns by using this equation:

Energy given out = 4.2_g-1C^-1 mass of water (g) its rise in temperature (ºC).

Then since you know what mass of fuel you burned you can work out the energy that would be given out by burning one mole of it.

The energy/heating/calorific value of a fuel refers to the amount of heat given out when a specific amount of fuel is burned.

Experiment

Aim: To find out the energy value of ethanol.

Materials: water, beaker, thermometer, weighing balance, spirit lamp and ethanol.

Procedure:

1. Pour a known volume of water into a beaker.
2. Measure the temperature of the water.
3. Fill the spirit lamp with enough ethanol.
4. Weight the mass of both the ethanol and the lamp.
5. Light the lamp and let it continue burning for a few minutes before putting it off.
6. Measure the water temperature again, to find the increase.
7. Reweigh the ethanol and its container to find how much ethanol was burned.

Record the following:

• Mass of spirit lamp + ethanol (initially)
• Mass of spirit lamp + ethanol (finally)
• Mass of ethanol burned
• Final temperature of water
• Initial temperature of water
• Rise in temperature of water
• Mass of water

The amount of heat (q) released by ethanol is given by:

Specimen calculation:

Mass of lamp and ethanol initially = 50g

Mass of lamp and ethanol finally = 49.5g

Mass of ethanol burned = 50.0 — 49.5 = 0.5g

Mass of water = 100g

Final temperature of water = 42ºC

Initial temperature of water = 20ºC

Rise in temperature = 42ºC – 20ºC = 22ºC

Specific heat capacity of water = 4.2 Jg^-1C^-1

Heat given out = Mass of water Xspecific heat capacity Xtemperature rise

Repeat similar procedures with kerosene, charcoal, coal, firewood etc. and compare your results. Which fuel has more energy per gram? That is the most efficient fuel.

How reliable is the experiment?

The following table compares the experimental results with values from data book.

Fuel	Heat of combustion in KJ/mol
	From the experiment	From a data book
Ethanol	-859	-1367
Butane	-1827	-2877

Note the big difference! The experimental results are almost 40% lower for both fuels. Why do you think there is such a big difference? There are two reasons for this:

1. Heat loss: Not all the heat from the burning fuel is transferred to the water. Some is lost to the air, and some to the container that holds the fuel.
2. Incomplete combustion: In case of a complete combustion, all the carbon in a fuel is converted to carbon dioxide. But here combustion is incomplete. Some carbon is deposited as soot on the bottom of the lamp and some converted to carbon monoxide. For example, when butane burns, a mixture of all these reactions may take place:

The less oxygen there is, the more carbon monoxide and carbon will form.