MEASURING ENERGY FROM FUELS

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Presentation transcript:

MEASURING ENERGY FROM FUELS CHEMISTRY N5 CHEMISTRY ENERGY FROM FUELS MEASURING ENERGY FROM FUELS

MEASURING ENERGY FROM FUELS CHEMISTRY N5 CHEMISTRY ENERGY FROM FUELS MEASURING ENERGY FROM FUELS After completing this topic you should be able to : Calculate the quantity of heat energy used to heat a given mass of water using the relationship Eh = cmΔT. Carry out an experiment to determine the heat energy Eh released from burning a fuel. State the measurements which are require to be made during the determination of the heat energy released from fuel experiment. Calculate Eh per gram of a fuel from experimental data.

MEASURING ENERGY FROM FUELS ENERGY RELEASED FROM FUELS Combustion of a fuel releases energy, i.e. it is an EXOTHERMIC REACTION. The unit for measuring energy is the JOULE (J). The unit is named after James Prescott Joule, the physicist who did a lot research on energy. A joule is a small quantity of energy. Often measurements of energy are given in kilojoules (kJ). To compare the quantity of energy released by different fuels the same mass of fuel must be burned in each experiment. The table shows the energy released when 1 gram of each fuel is burned. Energy released per gram (kJ g-1) Fuel How do chemists measure the energy released when 1 g of these fuels are burned? methane 55.7 butane 49.6 gasoline 48.3 methanol 22.7

Eh = c × m × ΔT MEASURING ENERGY RELEASED FROM A FUEL The energy released when a fuel burns can be used to heat water. When I absorb 418 kJ of energy from the flame, my temperature goes up by 1 oC. Facts about water: It requires 418 kJ of energy to raise 1 kilogram of water by 1 oC. This measurement is called the specific heat capacity of water. The symbol for this is the letter ‘c’. 1 cm3 of water has a mass = 1 g. Therefore, 1 kg of water has a volume = 1000 cm3 (1 litre). The energy required to heat a mass of water can be calculated using the following relationship: Eh = energy required to heat water in kJ. Eh = c × m × ΔT c = specific heat capacity of water = 418 kJ kg-1 oC-1. m = mass of water heated in kg. ΔT = temperature change of the water in oC.

Eh = c × m × ΔT Eh = c × m × ΔT = 418 × 05 × 16 Eh = 33.44 kJ Eh = energy required to heat water in kJ. c = specific heat capacity of water = 418 kJ kg-1 oC-1. m = mass of water in kg. ΔT = temperature rise of the water in oC. EXAMPLE Calculate the energy required to raise the temperature of 500 cm3 of water by 16 oC. Eh = c × m × ΔT c = 418 kJ kg-1 oC-1 = 418 × 05 × 16 m = 05 kg (500 cm3 = 500 g = 05 kg) ΔT = 16 oC Eh = 33.44 kJ Complete the HEATING WATER examples on page 2 of the MEASURING ENERGY FROM FUELS Examples Booklet.

MEASUREMENTS TO BE MADE EXPERIMENT: COMPARING FUELS AIM: To compare the energy released when 1 g of different alcohols is burned. ALCOHOLS: methanol, ethanol and propan-1-ol. thermometer MEASUREMENTS TO BE MADE copper can Mass of water in kg. Temperature of water before heating. Temperature of water after heating. Mass of burner at start. Mass of burner after heating water. 100 cm3 of water (0.1 kg) draught shield spirit burner fuel (alcohol) 100 cm3 of cold water is placed in the copper can and the temperature measured. The spirit burner is weighed before lighting. After lighting the burner, it is immediately placed under the can to heat the water. The water is stirred with the thermometer during heating. When the temperature of the water has risen by about 20 oC, the flame is extinguished, and the spirit burner weighed.

RESULTS ALCOHOL methanol ethanol propan-1-ol Mass of water / kg 0.1 Initial temperature of water / oC Final temperature of water / oC DT / oC Eh = c m DT (Energy transferred to the water) / kJ Initial mass of burner / g Final mass of burner / g Mass of alcohol burned / g Energy released per gram of alcohol / kJ g-1

CONCLUSION EVALUATION Look at the results of the experiment. Is there a pattern to the energy released when 1 g of methanol (CH3OH), ethanol (C2H5OH) and propan-1-ol (C3H7OH) is burned? EVALUATION Do you think your results are accurate? Do you think all the heat released from the burning fuels was transferred to the water? What are the limitations of the equipment? Can you suggest improvements to you could make to the experimental procedure? Complete the MEASURING ENERGY FROM FUELS examples on page 3 of the MEASURING ENERGY FROM FUELS Examples Booklet.