The bond enthalpy of N2(g) is 418.0 kJ/mol. Calculate ΔH°f for N(g).

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The bond enthalpy of N2(g) is 418.0 kJ/mol. Calculate ΔH°f for N(g).

The bond enthalpy of N₂(g) is 418.0 kJ/mol. Calculate ΔH°_f for N(g).

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Answer 1

Answer #1

Bond enthalpy is energy required to break a bond.

N2(g) -> 2 N(g) ΔH = 418.0 KJ/mol

Given:

ΔHo rxn = 418.0 KJ/mol

Hof(N2(g)) = 0.0 KJ/mol

Balanced chemical equation is:

N2(g) ---> 2 N(g)

ΔHo rxn = 2*Hof(N(g)) - 1*Hof( N2(g))

418.0 = 2*Hof(N(g)) - 1*(0.0)

Hof(N(g)) = -209 KJ/mol

Answer: -209 KJ/mol

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Answer 2

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The bond enthalpy of N2(g) is 418.0 kJ/mol. Calculate ΔH°f for N(g).

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The bond enthalpy of N2(g) is 418.0 kJ/mol. Calculate ΔH°f for N(g).