Write a balanced equation for the combustion of C7H16(l) (heptane) -- 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 C7H16(l) is -187.8 kJ/mol A) What is the standard heat of reaction (ΔH°) for the combustion reaction of C7H16(l)? B) Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of heptane.
Write a balanced equation for the combustion of C7H16(l) (heptane) -- 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 C7H16(l) is -187.8 kJ/mol A) What is the standard heat of reaction (ΔH°) for the combustion reaction of C7H16(l)? B) Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of heptane.
Chemistry: Principles and Practice
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Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
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Chapter5: Thermochemistry
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Write a balanced equation for the combustion of C7H16(l) (heptane)
-- 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 C7H16(l) is -187.8 kJ/mol
A) What is the standard heat of reaction (ΔH°) for the combustion reaction of C7H16(l)?
B) Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of heptane.
(Assume standard state conditions and 298 K for all reactants and products.)
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