To break the oxygen-oxygen bonds in a single O2 molecule, 1 * 10-18 J of energy is required. Which of the following wavelengths of light could be used to carry out this process?

E = hc / (lamda)

The lamda symbol is wavelength, which this site does not have. I can represent it with an "x" instead.

Plancks constant, h = 6.626*10^-32 J·s

Speed of light, c = 3.00*10^8 m/s

The energy must be greater than or equal to 1*10^-18 J

1*10^-18 J ≤ (6.626*10^-32 J·s) * (3.0*10^8 m/s) / x

x ≤ (6.626*10^-32 J·s) * (3.0*10^8 m/s) / (1*10^-18 J)

x ≤ 1.99*10^-7 m or 199 nm

The wavelength of light must be greater than or equal to 199 nm