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The energy required to break one mole of...

The energy required to break one mole of `Cl-Cl` bonds in `Cl_(2)` is `"242 kJ mol"^(-1)`. The longest wavelength of light capable of breaking a single `Cl-Cl` bond is
`(C=3xx10^(8)ms^(-1) and N_(A)=6.02xx10^(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 for breaking a `Cl_(2)` molecule
`= (242 xx 10^(3))/(N_(A))J = (242 xx 10^(3))/(6.02 xx 10^(23))J`
`E = (hc)/(lambda)` or `lambda = (hc)/(E)`
`= (6.626 xx 10^(-34) xx 3 xx 10^(8) xx 6.02 xx 10^(23))/(242 xx 10^(3))`
`= 494 xx 10^(-9) m = 494 nm`
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