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The energy required to break one mole of...

The energy required to break one mole of CI - Cl bonds in `Cl_(2)," is "242" kJ mol"^(-1)`. The longest wavelength of lig capable of breaking Cl-Cl bonds is `(c = 3 xx 10^(8)" ms"^(-1) and N_(A) = 6.02 xx 10^(23)" mol"^(-1))`

A

494 nm

B

594 nm

C

640 nm

D

700 nm

Text Solution

Verified by Experts

The correct Answer is:
A
Energy required to break `Cl_(2)` molecule `=(242xx10^(3))//N_(A)J`
From `E=hv rArr E="h"(c )/(lambda)" "` We have `lambda=(6.626xx10^(-34)xx3xx10^(8)xx6.022xx10^(23))/(242xx10^(3))=494.7nm`
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