Given that: (l)Δf H° of N2 O 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-1respectively, The resonance energy of N2 O is :

Question

Given that: (l)Δf H° of N2 O 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-1respectively, The resonance energy of N2 O is : (A) -88 kJ (B) -66 kJ (C) -62 kJ (D) -44 kJ

Tardigrade Admin · Accepted Answer

N2 (g)+(1/2) O2 → N2 O (g) N=N (g)+(1/2) (O=O →) Δ Hf0 = [Energy required for breaking of bonds] -[Energy released for forming of bonds] = (Δ HN=N +(1/2) Δ Ho=o - (Δ HN=N+Δ HN=O) = (946+(1/2)×498)-(418+607)=170 kJ mol-1 Resonance energy = 170-82 = 88 kJ mol-1

Q. Given that:
(l) $Δ_{f} H^{\circ} o f N_{2} O i s 82 K J m o l^{- 1}$
(ii) Bond energies of $N = N, N = N, O = O$ and $N = O$ are $946, 418, 498$ and $607 k J m o l^{- 1}$ respectively,
The resonance energy of $N_{2} O$ is :

$- 88 k J$

$- 66 k J$

$- 62 k J$

$- 44 k J$

Q. Given that: (l)Δf​H∘ofN2​Ois82KJmol−1 (ii) Bond energies of N=N,N=N,O=O and N=O are 946,418,498 and 607kJmol−1respectively, The resonance energy of N2​O is :

−88kJ

−66kJ

−62kJ

−44kJ

N2​(g)+21​O2​→N2​O(g) N=N(g)+21​(O=O→) ΔHf0​= [Energy required for breaking of bonds] -[Energy released for forming of bonds] =(ΔHN=N​+21​ΔHo=o​−(ΔHN=N​+ΔHN=O​) =(946+21​×498)−(418+607)=170kJmol−1 Resonance energy = 170-82 = 88 kJ mol−1

Q. Given that:
(l) $Δ_{f} H^{\circ} o f N_{2} O i s 82 K J m o l^{- 1}$
(ii) Bond energies of $N = N, N = N, O = O$ and $N = O$ are $946, 418, 498$ and $607 k J m o l^{- 1}$ respectively,
The resonance energy of $N_{2} O$ is :

$- 88 k J$

$- 66 k J$

$- 62 k J$

$- 44 k J$