Calculate the enthalpy change per mole of hydrazine combusted.?

Question

Hydrazine, N2H4, is a liquid used as a rocket fuel. It reacts with oxygen to yield nitrogen gas and water.

N2H4(λ) + O2(g) → N2(g) + 2 H2O(λ)

The reaction of 3.80 g N2H4 evolves 73.7 kJ of heat. Calculate the enthalpy change per mole of hydrazine combusted.

a.-8.98 × 103 kJ/mol
b.-622 kJ/mol
c.-8.74 kJ/mol
d.-19.4 kJ/mol
e.-2.80 × 102 kJ/mol

Answer 1

First, convert the mass of hydrazine into moles

Divide the kJ of heat released by the moles of hydrazine, and you should have it. (Recognize that your answer will be negative, since heat is evolved in the reaction.)

Answer 2

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