Calculate the resonance energy of N 2 O from the following data- - Hf of N 2 O-82 kJ mol -1- standard bond enthalpies of N - N - N - N- O - O and N - O bonds are 946- 418- 498 and KJ mol -1 respectively-

N≡ N+12O=O⟶ N=N=O Δ H^o_f=∑BE of reactants ∑BE of products #160; #160; #160; #160; #160; #160; =[BE(N≡ N)+12BE(O≡ O)] [BE(N=N)+B ...

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Bond Order and Enthalpy

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Calculate the resonance energy of $N_{2} O$ from the following data: $Δ H_{f}$ of $N_{2} O = 82 k J {m o l}^{- 1}$ , standard bond enthalpies of $N \equiv N$ , $N \equiv N$ , $O \equiv O$ and $N \equiv O$ bonds are 946, 418, 498 and $K J {m o l}^{- 1}$ respectively.

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N_{2} O

△_{f} H^{\circ}

N_{2} O = 82 k J m o l^{- 1}

N = N, N = N, O = O

N = O

946, 418, 498

607 k J m o l^{- 1}

N_{2} O

(Δ H_{f}^{o}

N_{2} O = 82 k J m o l^{- 1})

N_{2} O

Δ H_{f}^{\circ}

N_{2} O = 82 k J m o l e^{- 1}

N \equiv N

N = N

O = O

N = O

m o l e^{- 1}

N_{2} O

△ H_{f}^{o}

N_{2} O = 82 k J m o l^{- 1}

\equiv

k J m o l^{- 1}

N_{2} O

Δ H_{f}^{o}

N_{2} O = 134 K J {m o l}^{- 1}

N - O, N = O, N \equiv N

O = O

222, 607, 946

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

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