Sustainable Energy
2nd Edition
ISBN: 9781337551663
Author: DUNLAP, Richard A.
Publisher: Cengage,
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Textbook Question
Chapter 3, Problem 11P
The combustion of pure hydrogen by the reaction
produces 142 MJ per kg of hydrogen. Compare the energy per kg of octane and the total energy from the individual combustion of its carbon and hydrogen atoms.
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The change in internal energy for the combustion of 1.0 mol of octane at a pressure of 1.0 atm is -5084.3 kJ .
If the change in enthalpy is -5074.0 kJ , how much work is done during the combustion?
Express the work in kilojoules to three significant figures.
The Bunsen burner in your labs are fueled by natural gas, which is mostly methane, CH4. The
thermochemical equations for the combustion of methane (burning in oxygen) is:
CH4(g) + 2 O2(g) ➔ CO2(g) + 2 H2O (g) ΔH = – 890.3 kJ/mole
Calculate ΔH in kJ when 5.00 g CH4 react with an excess oxygen.
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.
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