Question

It takes 945 to break a nitrogen-nitrogen triple bond. Calculate the maximum wavelength of light for which a nitrogen-nitrogen triple bond could be broken by absorbing a single photon.

Answer 1

Answer: 127 nm

Explanation:

Given:

Energy required to break nitrogen-nitrogen bond = 945 kJ/mol =945000 J/mol

1 mole = $6.022\times 10^{23}$ molecules

$6.022\times 10^{23}$ molecules require energy to break nitrogen-nitrogen bond = 945000 kJ

1 molecule require energy to break nitrogen-nitrogen bond =$\frac{945000}{6.022\times 10^{23}}\times 1=1.569\times 10^{-18} kJ$

The relationship between wavelength and energy of the wave follows the equation:

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

where,

E= energy = $1.569\times 10^{-18} kJ$

h = Planck’s constant =$6.626\times 10^{-34}J$

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

$\lambda$ = wavelength of the wave = ?

Where,

$\lambda=\frac{h\times c}{E}=\frac{6.626\times 10^{-34}J\times 3\times 10^8 m/s}{1.569\times 10^{-18}J}=1.267\times 10^{-7} m=127nm$  

$(1nm=10^{-9}m$

Thus the maximum wavelength of light for which a nitrogen-nitrogen triple bond could be broken by absorbing a single photon is 127 nm