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Given that: (i) ΔH°...
 
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Given that: (i) ΔH°f of N2O is 82 kJ mol^-1 (ii) Bond energies of N ≡ N, N = N, O = O and N = O are 946, 418, 498 and 607 kJ mol^-1 respectively, The resonance energy of N2O is :

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Given that:

(i) ΔH°f of N2O is 82 kJ mol-1

(ii) Bond energies of N ≡ N, N = N, O = O and N = O are 946, 418, 498 and 607 kJ mol-1 respectively,

The resonance energy of N2O is :

(a) -88kJ

(b) -66kJ

(c) -62kJ

(d) -44kJ

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Correct answer: (a) -88kJ

Explanation:

N2(g) + 1/2O2 → N2O(g)

N ≡ N(g) + 1/2(O = O) → N = \(\overset{+}N\) = O(g)

ΔH°f = [Energy required for breaking of bonds]–[Energy released for forming of bonds]

= (ΔHN≡N + 1/2ΔHO=O - (ΔHN≡N + ΔHO=O))

= (946 + 1/2 x 498) - (418 + 607)

= 170 kJ mol-1

Resonance energy = 82 - 170

= -88 kJ mol-1

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