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  • Given that: (i) <img alt="\Delta _{f}H^{0} \, of N_{2}O \, is\, 82\, kJ\, mol^{-1}" src="https://entrancecorner.oncodecogs.com/gif.latex?%5CDelta%20_%7Bf%7DH%5E%7B0%7D%20%5C%2C%20of%

Given that:

(i) \Delta _{f}H^{0} \, of N_{2}O \, is\, 82\, kJ\, mol^{-1}

(ii) Bond energies of N\equiv N,N= N,O=O \, and\, N=O       

are\, 946,\: 418,\: 498\,\: \: and\:\; 607 kJ mol^{-1} respectively.

The resonance energy of N_{2}O is:

Option: 1

-88kJ


Option: 2

-66kJ


Option: 3

-62kJ


Option: 4

-44kJ


Answers (1)

best_answer

The enthalpy of formation of N_{2}O is given as 82 kJ/mol

The reaction could be written as.

N_{2}(g) +\frac{1}{2}O_{2}(g) \rightarrow N_{2}O(g)  

Now Calculating bond dissociation enthalpy, \Delta _{cal}H = \sum Reactants - \sum Products

\Delta _{cal}H = (946 + \frac{1}{2}498) - (418+607)

\Delta _{cal}H = 170\; kJ/mol

Resonance energy = Observed heat of formation - Calculated heat of formation

Resonance energy = 82 - 170 = -88 kJ/mol

Posted by

vinayak

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