It takes 945kJ/mol to break a nitrogen nitrogen triple bond calculate the maximum wavelength of light for which a nitrogen nitrogen triple bond could be broken by absorbing a single photon

Question

Be sure your answer has correct number of significant digits in nm

Answer 1

To calculate the maximum wavelength of light for breaking a nitrogen-nitrogen triple bond, we can use the equation:

E = hc/λ

where E is the energy in Joules, h is the Planck constant (6.626 x 10^-34 J*s), c is the speed of light (2.998 x 10^8 m/s), and λ is the wavelength in meters.

First, we need to convert the energy from kilojoules per mole (kJ/mol) to Joules per molecule (J). Since we are considering a single molecule, we divide 945 kJ/mol by Avogadro's number (6.022 x 10^23 molecules/mol) to get the energy per molecule:

E = (945 kJ/mol / 6.022 x 10^23 molecules/mol) = 1.571 x 10^-21 J

Next, we can solve the equation for λ:

λ = hc/E

λ = (6.626 x 10^-34 J*s * 2.998 x 10^8 m/s) / (1.571 x 10^-21 J)

λ = 1.261 x 10^-6 m

Finally, we convert the wavelength from meters to nanometers by multiplying by 10^9:

λ = 1.261 x 10^-6 m * 10^9 nm/1 m = 1.261 nm

Therefore, the maximum wavelength of light for which a nitrogen-nitrogen triple bond could be broken by absorbing a single photon is approximately 1.261 nm.