Hydrazine, N2H4, decomposes according to the following reaction: (a) Given that the standard enthalpy of formation of
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(a) Given that the standard enthalpy of formation of hydrazine is 50.42 kJ/mol, calculate (H° 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 (H° for each of them. On a mass basis (per kg), would hydrazine or ammonia be the better fuel?
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a b The balanced equations are The standard enthalpy change for equation 1 is The standa...View the full answer
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