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The bond dissociation energies of $N \equiv N, N = N, O = O & N = O$ are 946, 418, 498 and 607 KJ/mole respectively. If heat of formation of $N_{2} O$ is 82 KJ/mole then the magnitude of resonance energy of $N_{2} O$ in KJ/mole is__

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92 KJ/mole

88 KJ/mole

83 KJ/mole

78.5 KJ/mole

answer is C.

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Detailed Solution

$N \equiv N + \frac{1}{2} (O = O) \to N = N = O; Δ H f (c a l) = ?$

$Δ H = \sum_{}^{} [B D E (R) - B D E (P)]$

$Δ H f (c a l) = (946 + \frac{498}{2}) - (418 + 607)$

$Δ H f (c a l) = 170 K J / m o l e$

$Δ H f (E x p t) = 82 K J / m o l e$

Resonance Energy $= Δ H f (c a l) - Δ H f (E x p t)$

$R E = 170 - 82$

$R E = 88 K J / m o l e$

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