Question

It takes 338. kJ/mol to break an carbon-chlorine single bond. Cal broken by absorbing a single photon Iculate the maximum wavelength of light for which an carbon-chiorine single bond could be Round your answer to 3 significant digits

Answer 1

354 nm

Step-by-step explanation:

`E=(h* c)/(\lambda)`

Where,

h is Plank's constant having value
`6.626* 10^(-34)\ Js`

c is the speed of light having value
`3* 10^8\ m/s`

`\lambda` is the wavelength of the light

So, Given that:- Energy = 338. kJ/mol = 338000 J/mol

Also,
`N_a=6.023* 10^(23)\ {mol}^(-1)`

So, Energy for single photon =
`(338000)/(6.023* 10^(23))\ J`

Applying the values in the above equation as:-

`(338000)/(6.023* 10^(23))=(6.626* 10^(-34)* 3* 10^8)/(\lambda)`

`69* \:10^(26)\lambda=5^(20)* \:62770482.511`

`\lambda=354* 10^(-9)\ m=354\ nm`