Sustainable Energy
2nd Edition
ISBN: 9781337551663
Author: DUNLAP, Richard A.
Publisher: Cengage,
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Chapter 6, Problem 20P
To determine
Find the mass and volume of spent from commercial power reactors.
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Assume that gasoline is burned with 99% efficiency in a car engine, with 1% remaining unbumed in the exhaust gases as VOCs; If the engine exhausts 16 kg of gases (MW = 30) for each kg of gasoline (MW = 100), calculate the fraction of VOCs in the exhaust. Give your answer in parts per million.
1) Heating the water in a 55-gallon water heater requires about 2.0 x 103 kJ of energy.
a) Assume the energy came from natural gas with 80% efficiency; how many grams of natural gas are required?
b) Assume the energy came from electricity with 80% efficiency and that the electricity was produced from the combustion of coal with 30% efficiency; how many grams of coal are required?
For problem above, calculate how much CO2 in grams is emitted to the atmosphere.
For a: Use the balanced equation for the combustion of methane (CH4) to determine how many grams of CO2are produced from the amount of natural gas required.
For b: Assume that coal produces 5.25 kJ of energy per gram of CO2 produced. Calculate how much CO2 in grams is produced.
Calculate the total mass of CO2 in the atmosphere. State all assumptions. Compare this to the actual of ~3.6 ×1012 tonnes. At our current rate of emissions, how long would it take to emit a quantity equal to the present mass of CO2 in the atmosphere
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- One gram of methane is burned, and the heat is used to raise the temperature of 1 kg of water. If the initial temperature of the water is 25C, what is the final temperature?arrow_forwardA new coal-fired power plant has been built using a sulfur emission control system that is 70 percent efficient. If all of the sulfur oxidizes to SO2 and if the emission of SO2 are lmited to 0.6 lb SO2 per million Btu of heat into the power plant, what maximum percent sulfur content can the fuel have if 15,000 Btu/lb coal is burned?arrow_forwardA simple way of looking at the energy associated with the combustion of methane [as shown in equation (1.15)] is to view the oxidation of the carbon by equation (1.13) and the oxidation of hydrogen by equation (1.19). Based on the energies involved in these processes, discuss the validity of this approach.arrow_forward
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