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/molΔHf° of H2O(l) is -286 kJ/molΔHf° of C9H20(l) is -229.0 kJ/mol-6172.5 kJCalculate 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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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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:

ΔH_f° of CO₂(g) is -393.5 kJ/mol
ΔH_f° of H₂O(l) is -286 kJ/mol
ΔH_f° 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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