Write a balanced equation for the combustion of C9H20(l) (nonane)-- i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l). Given the following standard heats of formation: ΔHf° of CO2(g) is -393.5 kJ/mol ΔHf° of H2O(l) is -286 kJ/mol ΔHf° of C9H20(l) is -229.0 kJ/mol -6172.5 kJ Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of nonane.(Assume standard state conditions and 298 K for all reactants and products.)
Write a balanced equation for the combustion of C9H20(l) (nonane)-- i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l). Given the following standard heats of formation: ΔHf° of CO2(g) is -393.5 kJ/mol ΔHf° of H2O(l) is -286 kJ/mol ΔHf° of C9H20(l) is -229.0 kJ/mol -6172.5 kJ Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of nonane.(Assume standard state conditions and 298 K for all reactants and products.)
Chemistry by OpenStax (2015-05-04)
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Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
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Chapter16: Thermodynamics
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Problem 56E: Nitric acid, HNO3, can be prepared by the following sequence of reactions:...
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Write a balanced equation for the combustion of C9H20(l) (nonane)
-- i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l).
Given the following standard heats of formation:
- ΔHf° of CO2(g) is -393.5 kJ/mol
- ΔHf° of H2O(l) is -286 kJ/mol
- ΔHf° of C9H20(l) is -229.0 kJ/mol
-6172.5 kJ
Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of nonane.
(Assume standard state conditions and 298 K for all reactants and products.)
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