Question

It takes to break an iodine-iodine single bond. Calculate the maximum wavelength of light for which an iodine-iodine single bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits.

Answer 1

The given question is incomplete. The complete question is :

It takes 151 kJ/mol to break an iodine-iodine single bond. Calculate the maximum wavelength of light for which an iodine-iodine single bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits.

Answer:  793 nm

Explanation:

The relation between energy and wavelength of light is given by Planck's equation, which is:

$E=\frac{hc}{\lambda}$

where,

E = energy of the light  = 151 kJ= 151000 J   (1kJ=1000J)

N= moles = 1 = $6.023\times 10^{23}$

h = Planck's constant  = $6.626\times 10^{-34}Js$

c = speed of light  = $3\times 10^8m/s$

$\lambda$ = wavelength of light  = ?

Putting in the values:

$151000J=\frac{6.023\times 10^{23}\times 6.626\times 10^{-34}Js\times 3\times 10^8m/s}{\lambda}$

${\lambda}=7.93\times 10^{-7}m=793nm$    $1m=10^{-9}nm$

Thus  the maximum wavelength of light for which an iodine-iodine single bond could be broken by absorbing a single photon is 793 nm