Answer;
Wavelength= 1197.47 nm
Explanation and solution;
1.0x10^2 kJ/mole x (1 mole / 6.022x10^23 photons) x (1000 J / 1 kJ)
= 1.66 x10^-19 J/photon
Energy of a wave = ħc / λ
where;
E = energy of the wave = = 1.66 x10^-19 J/photon
ħ = plancks constant = 6.626x10^-34 J s
c = speed of light = 3.00x10^8 m/s
λ = wavelength
λ = ħc / E
= (6.626x10^-34 J s) x (3.00x10^8 m/s) / (1.66 x10^-19 J)
λ = 1.197 x10^-6 m x (1x10^9 nm / m)
= 1197.47 nm
