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The bond dissociation energies of X2, Y2...

The bond dissociation energies of `X_2, Y_2 and XY` are in the ratio of `1 : 0.5 : 1. DeltaH` for the formation of XY is -200 kJ mol^(-1)`. The bond dissociation energy of `X_2` will be

A

`"100 kJ mole"^(-1)`

B

`"800 kJ mole"^(-1)`

C

`"300 kJ mole"^(-1)`

D

`"400 kJ mole"^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
B
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Knowledge Check

  • Enthalpy change for the reaction, 4H(g) to 2H_2(g) is -869.6 kJ The dissociation energy of H - H bond is

    A
    `-869.6 kJ`
    B
    ` + 434.8 kJ`
    C
    ` +217.4 kJ`
    D
    `-434.8 kJ`

  • The bond dissociation energy of B-F in BF_(3) is 646 kJ mol^(-1) whereas that of C-F in CF_(4) is 515 kJ mol^(-1) . The correct reason for higher B-F bond dissociation energy as compared to that of C-F in CF_(4) is

    A
    stronger `sigma` bond between B and F in `BF_(3)` as compared to that between C and F in `CF_(4)`
    B
    significant `p pi- p pi` interaction between B and F in `BF_(3)` whereas there is no possibility of such interaction between C and F in `CF_(4)`
    C
    lower degree of `p pi- p pi` interaction between B and F in `BF_(3)` than that between C and F in `CF_(4)`
    D
    smaller size of B - atoms as compared to that of C-atom