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The H-H bond energy is 430 kJ mol^(-1) a...

The H-H bond energy is 430 kJ `mol^(-1)` and Cl-Cl bond energy is 240 kJ `mol^(-1)`, `DeltaH and HCl` is -90kJ. The H-Cl bond energy is about

A

180 kJ `mol^(-1)`

B

360 kJ `mol^(-1)`

C

213 kJ `mol^(-1)`

D

425 kJ `mol^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
D
The formation of one mole of HCl can be represented as, `(1)/(2)(H-H)+(1)/(2)(Cl-Cl)toH-Cl,DeltaH=-90kJ`
Hence, for the reaction,
Heat evolved=heat evolved in bond formation-heat required for bond breaking
`therefore 90 kJ=[H-Cl" bond energy"]-((1)/(2)xx430+(1)/(2)xx240)`
`therefore(H-Cl" bond energy")=90+(215+120)=425" kJ "mol^(-1)`
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Knowledge Check

  • The H-H bond energy is 430KJmol^(-1) and Cl-Cl bond energy is 240KJmol^(-1) . DeltaH for HCl is -90KJ . The H-Cl bond energy is about

    A
    `425KJmol^(-1)`
    B
    `213KJmol^(-1)`
    C
    `306KJmol^(-1)`
    D
    `180KJmol^(-1)`

  • The H-H bond energy is 430KJ mol^(-1) and Cl-Cl bonds is 240KJ mol^(-1) . DeltaH for HCl is -90KJ . The H-Cl bond energy is about.

    A
    `425KJmol^(-1)`
    B
    `KJmol^(-1)`
    C
    `360mol^(-1)`
    D
    `180mol^(-1)`

  • From the following bond energies H-H bond energy : 431.37 kJ mol^(-1) C=C bond energy : 606.10 kJ mol^(-1) C-C bond energy : 336.49 kJ mol^(-1) C-H bond energy : 410.50 kJ mol^(-1) Enthalpy for the reaction. underset(H)underset(|)overset(H)overset(|)(C)=underset(H)underset(|)overset(H)overset(|)(C)+H-HrarrH-underset(H)underset(|)overset(H)overset(|)(C)-underset(H)underset(|)overset(H)overset(|)(C)-H will be

    A
    1523.6 kJ `mol^(-1)`
    B
    `-243.6 kJ mol^(-1)`
    C
    `-120.0 kJ mol^(-1)`
    D
    553.0 kJ `mol^(-1)`

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