ThermochemistryHard
Question
The standard heat of combustion of propane is −2220.1 kJ/mol. The standard heat of vaporization of liquid water is 44 kJ/mol. What is the ΔHo of the following reaction?
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)
Options
A.−2220.1 kJ
B.– 2044.1 kJ
C.−2396.1 kJ
D.−2176.1 kJ
Solution
$\Delta H^{o} = ( - 2220.1) + 4 \times 44 = - 2044.1\text{ kJ}$
Create a free account to view solution
View Solution FreeMore Thermochemistry Questions
Among the following, for which reaction the heat of reaction represents bond energy of HCl?...Calculate proton affinity of NH3(g) from the following data.ΔHdissociation H2 = 218 kJ mole–1ΔHdissociation Cl2 = 124 kJ...For the given reactionsSiO2 + 4HF → SiF4 + 2H2O, ᐃH = -10.17 kcalSiO2 + 4HCl → SiCl4 + 2H2O, ᐃH ...The enthalpy change in a reaction does not depend upon...Standard molar enthalpy of formation of CO2 is equal to...