To calculate the maximum wavelength of light needed to break an oxygen-hydrogen single bond, we can use the equation:
E = hc/λ
Where:
E = energy required to break the bond (in J)
h = Planck's constant = 6.62607015 × 10^-34 J·s
c = speed of light in vacuum = 2.998 × 10^8 m/s
λ = wavelength of light (in meters)
First, let's convert the energy required from kJ/mol to J/molecule:
1 kJ/mol = 1 kJ/ (6.022 × 10^23 molecules)
463 kJ/mol = (463 × 10^3 J) / (6.022 × 10^23 molecules)
463 kJ/mol = 7.686 × 10^-19 J/molecule
Now we can calculate the maximum wavelength:
E = hc/λ
7.686 × 10^-19 J/molecule = (6.62607015 × 10^-34 J·s)(2.998 × 10^8 m/s) / λ
Rearranging the equation to solve for λ:
λ = (6.62607015 × 10^-34 J·s)(2.998 × 10^8 m/s) / (7.686 × 10^-19 J/molecule)
Calculating the maximum wavelength:
λ ≈ 2.5885852 × 10^-7 meters
Converting meters to nanometers:
λ ≈ 2.5885852 × 10^-7 meters * (10^9 nm/1 meter)
λ ≈ 258.85852 nm
Therefore, the maximum wavelength of light required to break an oxygen-hydrogen single bond is approximately 258.9 nm (rounded to the correct number of significant digits).
It takes 463 kJ/mol to break an oxygen hydrogen single bond calculate the maximum wavelength of light which an oxygen hydrogen single bond could be broken by absorbing a single photon
Be sure your answer has correct number of significant digits in nm
1 answer