1. Use tabulated standard enthalpies of formation to calculate a theoretical value for the molar enthalpy of combustion of acetone.
Here is what I have so far....
Write a balanced equation: C3H6O(l) + 4O2(g) --> 3CO2(g) + 3H2O(l)
Under each compound, write out the enthalpy of formation, ignoring the number of moles.
C3H6O(l) + 4O2(g) --> 3CO2(g) + 3H2O(l)
- -0.0 -393.5 -285.8
I know i need to use this formula but can someone tell me how to sub in my values in to this formula?
∆H = ∑n∆H°f(prod.) - ∑n∆H°f(react.)