It takes 157./kjmol to break a nitrogen-oxygen single bond. calculate the maximum wavelength of light for which a nitrogen-oxygen single bond could be broken by absorbing a single photon. round your answer to 3 significant digits.

Energy E = 157 kjmol

We have Avogadro constant Na = 6.023 Ă - 10^23/mol

Planck constant, h = 6.626 Ă - 10^-34 J s

Speed of light, Vl = 3.00 Ă - 10^8 m/s = lambda x V

We have energy E = Na x h x V = > E = Na x h x (Vl / lambda)

157 x 10^3 = (6.023 Ă - 10^23 x 6.626 Ă - 10^-34 x 3.00 Ă - 10^8) / lambda

lambda = (6.023 Ă - 10^23 x 6.626 Ă - 10^-34 x 3.00 Ă - 10^8) / 157 x 10^3

lambda = 119.72 x 10^-3 / 157 x 10^3 = 0.76258 x 10^-6 m

Wavelength = 763 nm