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If DeltaH(f)^(@) of Icl(g), Cl(g) and I(...

If `DeltaH_(f)^(@)` of `Icl(g)`, `Cl(g)` and `I(g)` is `17.57`, `121.34` and `106.96 J mol^(-1)` respectively. Then bond dissociation energy of `I-Cl` bond is

A

`35.15 J mol^(-1)`

B

`106.69 J mol^(-1)`

C

`210.73 J mol^(-1)`

D

`420.9 J mol^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
C
`I(g) + Cl(g) to Cl(g) " "Delta H_(f) (IC l) = 17.57 J//mol`
`121.34 + 106.96 - (I - Cl) = 17.57`
`121.34 + 106.96 - 17.57 = ( I - Cl)`
Bond dissociation (I - Cl) bond `= 210.73 J//mol`.
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