To calculate the maximum wavelength of light for breaking a nitrogen-oxygen single bond, use the equation λmax = hc/E, where E is the bond energy. Convert the bond energy to joules and solve for λmax. Multiply the result by 10^9 to get the maximum wavelength in nanometers.
To calculate the maximum wavelength of light for which a nitrogen-oxygen single bond could be broken by absorbing a single photon, we need to determine the energy required to break the bond. The energy required to break a bond can be calculated using the equation E = hc/λ, where E is the energy, h is Planck's constant (6.626 x 10^-34 J·s), c is the speed of light (3.00 x 10^8 m/s), and λ is the wavelength of light.
Let's assume that the maximum wavelength for breaking the bond is λmax. Rearranging the equation, we have λmax = hc/E. Plugging in the values h = 6.626 x 10^-34 J·s and E = bond energy, we can calculate λmax in meters. To convert it to nanometers, we multiply the result by 10^9.
For example, if the bond energy is 200 kJ/mol, we first convert it to joules by dividing by Avogadro's number (6.022 x 10^23/mol) and multiplying by 1000 to convert kJ to J. Then we calculate λmax = (6.626 x 10^-34 J·s * 3.00 x 10^8 m/s) / (200 x 10^3 J/mol / (6.022 x 10^23/mol)) * 10^9. This will give us the maximum wavelength of light in nanometers.
The complete question is- nitrogen-oxygen single bond. How to calculate the maximum wavelength of light for which a nitrogen-oxygen single bond could be broken by absorbing a single photon.