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
The intermediate SiH2 is formed in the thermal decomposition of silicon hydrides. Calculate ΔHf° of SiH2 from the follow...Match the transformations in column I with appropriate options in column II...Among the following, for which reaction the heat of reaction represents bond energy of HCl?...The enthalpy change in a reaction does not depend upon...CsF(S) → Cs+(aq) + F-(aq) ᐃH = - 40 kJ mol- If lattic energy of CsF is 750 kJ mol- . Then the summation of h...