Sustainable Energy
2nd Edition
ISBN: 9781337551663
Author: DUNLAP, Richard A.
Publisher: Cengage,
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Chapter 4, Problem 7P
To determine
Find the gasoline required to burn to reach a lethal level of carbon monoxide.
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Q3: B:
A 208 g of C6H6 (78 g/mol.) burns in air according to the equation:
CHs + O2 - CO2 +H2O
What mass of CO2 (44 g/mol.) is produced?
The enthalpy of combustion of benzoic acid (C6 H5 COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be −3226.7 kJ/mol. When 1.9862 g of benzoic acid are burned in a calorimeter, the temperature rises from 21.84°C to 25.67°C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2000 g.)
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.
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