Octane (C8H18) undergoes combustion according to the following thermochemical equation: 2C8H18(l) + 25O2(g) → 16CO2(g) + 18H2O(l), ΔH°rxn = –11,020 kJ/mol. Given that ΔH°f[CO2(g)] = –393.5 kJ/mol and ΔH°f[H2O(l)] = –285.8 kJ/mol, calculate the standard enthalpy of formation of octane. –11,230 kJ/mol 22,040 kJ/mol 420 kJ/mol –210 kJ/mol –420 kJ/mol
Octane (C8H18) undergoes combustion according to the following thermochemical equation: 2C8H18(l) + 25O2(g) → 16CO2(g) + 18H2O(l), ΔH°rxn = –11,020 kJ/mol. Given that ΔH°f[CO2(g)] = –393.5 kJ/mol and ΔH°f[H2O(l)] = –285.8 kJ/mol, calculate the standard enthalpy of formation of octane. –11,230 kJ/mol 22,040 kJ/mol 420 kJ/mol –210 kJ/mol –420 kJ/mol
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
Problem 99QRT
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Question
Octane (C8H18) undergoes combustion according to the following thermochemical equation:
2C8H18(l) + 25O2(g) → 16CO2(g) + 18H2O(l), ΔH°rxn = –11,020 kJ/mol.
Given that ΔH°f[CO2(g)] = –393.5 kJ/mol and ΔH°f[H2O(l)] = –285.8 kJ/mol, calculate the standard enthalpy of formation of octane.
–11,230 kJ/mol
|
||
22,040 kJ/mol
|
||
420 kJ/mol
|
||
–210 kJ/mol
|
||
–420 kJ/mol
|
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