Chemistry
posted by Patsy on .
3 N2H4(g)+N2O4(g)¨ 4 N2(g) + 4H2O(g) + 2 H2(g)
∆H= 1310 kJ (312 kcal)
How much energy is produced per mole of hydrazine burned?
a. 13.6 kJ (3.25kcal)
b. 40.9 kJ (9.75kcal)
c. 437 kJ (104kcal)
d. 1310 kJ (312 kcal)

My assumption is that this reaction, as written, produces 1310 kJ heat. That's for 3 mols N2H4; therefore, 1 mol would be just 1/3 of that. Right?