Question

It takes 238./kjmol to break a carbon-iodine single bond. calculate the maximum wavelength of light for which a carbon-iodine single bond could be broken by absorbing a single photon. round your answer to 3 significant digits.

Answer 1

Answer : wavelength will be 502 nm

Given data is

Energy = 238 kJ so, in Joules it will be = 238,000J.

To calculate in terms of moles we need to divide it will avogadro's number

238000 / (6.022 X $10^{23}$) = 3.953$10^{-19}$ J

we have the energy formula as E = hνc = λν ;

as we know the value of E, we can modify the equation as E = hc/λ

and rearrange it into λ = hc/E

on solving we get,

(6.626$10^{-34}$ Js X 2.9979$10^{8}$m/s) / (3.953$10^{-19}$ )

we get answer as = 5.02$10^{-7}$ m

for nm we have to multiply by 1nm/1$10^{-9}$ m

So, the answer is = 502 nm