Answer: Hydrazine, N2H4, decomposes according to the
Chapter 6, Problem 6.76(choose chapter or problem)
Hydrazine, N2H4, decomposes according to the following reaction: 3N2H4(l) 4NH3(g) 1 N2(g) (a) Given that the standard enthalpy of formation of hydrazine is 50.42 kJ/mol, calculate DH8 for its decomposition. (b) Both hydrazine and ammonia burn in oxygen to produce H2O(l) and N2(g). Write balanced equations for each of these processes and calculate DH8 for each of them. On a mass basis (per kg), would hydrazine or ammonia be the better fuel?
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