Consider the formation enthalpy of hydrazine (N2H4) according to the balanced chemical equation:
N2(s) + 2 H2(g) ? N2H4(g)
Derive the standard enthalpy of formation of hydrazine from the following known standard enthalpies:
H2O(g) ? H2O(l) ?Hcon = -44 kJ
2 H2(g) + O2(g) ? 2 H2O(l) ?Hrxn = -572 kJ
2 N2H4(g) + 7 O2(g) ? 2 N2O5(s) + 4 H2O(g) ?Hrxn = -1154 kJ
2 N2(s) + 5 O2(g) ? 2 N2O5(s) ?Hrxn = 101.2 kJ
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