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

Ch4 is nonpolar and insoluble in water. since all of the hydrogen atoms are evenly spread around the carbon atom even through the c h bond is polar all the poles cancel each other out.