Based on the values of bond energies given- - fHo of N2H4g is- Given- N - N - 159 kJ mol-1 - H - H - 436 kJ mol-1 N - N - 941 kJ mol-1 - N - H - 398 kJ mol-1

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Heat of Reaction

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Based on the values of bond energies given, $Δ_{f} H^{o}$ of $N_{2} H_{4} (g)$ is:
Given: $N - N = 159 {kJ mol}^{- 1}; H - H = 436 {kJ mol}^{- 1}$
$N \equiv N = 941 {kJ mol}^{- 1}; N - H = 398 {kJ mol}^{- 1}$

700 k J m o l^{- 1}

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62 k J m o l^{- 1}

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- 98 k J m o l^{- 1}

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- 711 k J m o l^{- 1}

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Δ_{f} H^{o}

N_{2} H_{4} (g)

N - N = 159 {kJ mol}^{- 1}; H - H = 436 {kJ mol}^{- 1}

N \equiv N = 941 {kJ mol}^{- 1}; N - H = 398 {kJ mol}^{- 1}

(B . E .)

Δ_{f} H^{\circ}

N_{2} H_{4} (g)

N - N = 159 {kJ mol}^{- 1}; H - H = 436 {kJ mol}^{- 1} N \equiv N = 941 {kJ mol}^{- 1}; N - H = 398 {kJ mol}^{- 1}

ϵ_{N \equiv N} = 945 {kJ mol}^{- 1}, ϵ_{H - H} = 436 {kJ mol}^{- 1}

ϵ_{(N - H)} = 391 {kJ mol}^{- 1}

N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)

Δ_{f} H^{0}

N_{2} H_{4} (g)

N - N = 159 k J m o l^{- 1}; H - H = 436 k J m o l^{- 1}

N \equiv N = 941 k J m o l^{- 1}; {N - H = 398 k J m o l}^{- 1}

N_{2} O

△ H^{\circ} (N_{2} O) = 82 k J m o l^{- 1}

N^{Θ} = N^{⨁} = O

(N \equiv N) b o n d = 950 k J m o l^{- 1}

(N = N) b o n d = 420 k J

^{- 1}

O = O) b o n d = 500 k J m o l^{- 1}

(O = N) b o n d = 610 k J m o l^{- 1}

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