The energy from the combustion of Hydrazine, N2H4, is used to power rockets into space in the reaction:
N2H4(g)+O2(g)=N2(g)+2H2O(l) delta H degree= -627.6KJ
How many killograms of hydrazine would be necessary to produce 1.0 X 10^8 KJ of energy?
Hint: One mole of N2H4 produces 627.6KJ of energy. How many moles (and then grams) are required to produce 1.0 X 10^8 KJ of energy.
MM(N2H4)= 32.04 g/mol
Answer: 5105 kg