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If the bond enthalpy of O(2),N(2)" and "...

If the bond enthalpy of `O_(2),N_(2)" and "H_(2)` are 498, 946 and 435.8 kJ `mol^(-1)` respectively. Choose the correct order of decreasing bond strength.

A

`H_(2)gtN_(2)gtO_(2)`

B

`N_(2)gtO_(2)gtH_(2)`

C

`O_(2)gtH_(2)gtN_(2)`

D

`H_(2)gtO_(2)gtN_(2)`

Text Solution

Verified by Experts

(b) Larger the bond dissociation enthalpy, stronger will be the bond in the molecule.So, `{:(N_(2),gt,O_(2),gt,H_(2)),(946 kJ mol^(-1),,498 kJ mol^(-1),,435.8 kJ mol^(-1)):}`
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Knowledge Check

  • Bond dissociation enthalpy of H_(2), Cl_(2) and HCl are 434, 242 and 431 kJ mol^(-1) respectively. Enthalpy of formation of HCl is

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