Asked by Ruth
Hydrazine has the formula N2H4 and is used as a rocket fuel (e.g. for the Apollo moon rockets). It burns in the following reaction for which the enthalpy change is -583 kJ/mol.
N2H4(g) + O2(g) → N2(g) + 2 H2O(g)
Calculate the N-N bond enthalpy in hydrazine given the following bond enthalpies.
Bond enthalpies: N-H 388, O=O 498, NòN 944, O-H 463 kJ/mo
N2H4(g) + O2(g) → N2(g) + 2 H2O(g)
Calculate the N-N bond enthalpy in hydrazine given the following bond enthalpies.
Bond enthalpies: N-H 388, O=O 498, NòN 944, O-H 463 kJ/mo
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Answered by
Sam
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