Write a balanced equation for the combustion of CH3C6H13(l) (methyl hexane)-- 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 CH3C6H13(l) is -173.0 kJ/molWhat is the standard heat of reaction (ΔH°) for the combustion reaction of CH3C6H13(l)?Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of methyl hexane. (Assume standard state conditions and 298 K for all reactants and products.)

Given Reaction:- CH3C6H13(l) + 11O2 ------> 7CO2(g) + 8H2O ΔHf° of CO2(g) is -393.5 kJ/mol ΔHf°…

Answered: Write a balanced equation for the…

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

Section4.7: Where Does The Energy Come From?

Problem 4.13CE

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Write a balanced equation for the combustion of CH₃C₆H₁₃(l) (methyl hexane)
-- 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 CH₃C₆H₁₃(l) is -173.0 kJ/mol

What is the standard heat of reaction (ΔH°) for the combustion reaction of CH₃C₆H₁₃(l)?

Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of methyl hexane.
(Assume standard state conditions and 298 K for all reactants and products.)

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