It takes 163./kjmol to break an nitrogen-nitrogen single bond. calculate the maximum wavelength of light for which an nitrogen-nitrogen single bond could be broken by absorbing a single photon. be sure your answer has the correct number of significant digits.

Answer is:  the maximum wavelength of light is 7.34 × 10⁻⁷ m.

E= 163 kJ/mol; bond energy of one mole of nitrogen.

E = 163000 J/mol ÷ 6.022·10²³ 1/mol.

E = 2.707·10⁻¹⁹ J; bond energy per molecule.

E = h·c/λ.

c = 3.00 × 10⁸ m/s; light speed.

h = 6.62607004·10⁻³⁴ J·s; Planck constant.

λ(photon) = h·c/E.

λ(photon) = 6.62607004·10⁻³⁴ J·s · 3.00 × 10⁸ m/s ÷ 2.707·10⁻¹⁹ J.

λ(photon) = 7.34 × 10⁻⁷ m.

λ(photon) = 734 nm.

im not exactly sure but i think its b!

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.