# Chemistry

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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)

• Chemistry -

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?

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