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19 March, 01:20

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.

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  1. 19 March, 03:29
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    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
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