Question: Use tabulated standard enthalpies of formation to calculate a theoretical value for the molar enthalpy of combustion of acetone.
THE FOLLOWING IS MY WORK PLEASE TELL ME IF THERE ARE ANY MISTAKES. THANK YOU
1. Write a balanced equation: C3H6O(l) + 4O2(g) --> 3CO2(g) + 3H2O(l)
2. Under each compound, write out the enthalpy of formation, ignoring the number of moles.
C3H6O(l) + 4O2(g) --> 3CO2(g) + 3H2O(l)
-248.1 0.0 -393.5 -285.8
3. Put the enthalpy values into the equation but now you have to take the number of moles into account:
∆H = ∑n∆H°f(prod.) - ∑n∆H°f(react.)
= [3(-393.5) + 3(-285.
] – [(-248.1) + 4(0.0)] kJ/mol
= [-2037.9 – (-248.1)] kJ/mol
= -1789.8 kJ/mol