Write a balanced equation for the combustion of C5H12(l)(pentane)
— 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 C5H12(l)is -146.4 kJ/mol
What is thestandard heat of reaction(ΔH°) for the combustion reaction of C5H12(l)?
-3537.1 kJ ( i got this one)
Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of pentane. (Assume standard state conditions and 298 K for all reactants and products.)