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

Options

A. 180 kJ `mol^(-1)`
B. 360 kJ `mol^(-1)`
C. 213 kJ `mol^(-1)`
D. 425 kJ `mol^(-1)`

Answer

D

Explanation

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)`