Question

I found deltaH to be -115.3 kJ, but it is wrong. I found moles ofthe each component and multiplied by respected heats of formation,then took products-reactants. I do not understand what went wrong.Please explain in detail how to find deltaH, I think I can find therest out by myself afterwards.


Determine H, q, w, and E at 298 K and 1 atm for the completereaction of 8.090 g of N2O4.
N2O4(g) + 2N2H4(l) 3N2(g) + 4H2O(l).
The heat of formation of liquid hydrazine (N2H4) is 50.63 kJ/mol.Use tabulated data for other heats of formation.
The tolerance on each question is only 0.03 kJ, so express allanswers to 0.01 kJ.
deltaH = kJ
q = kJ
w = kJ
deltaE = kJ