What is the energy in kJ/mol of photons with a wavelength of 450 nm?

If 310 kJ/mol of energy is required to make the reaction proceed, what wavelength of light is necessary to provide this energy?

The energy of a single photon is 2.441 × 10⁻²⁰ J. What is the energy of one mole of these photons, in kilojoules?

Ultraviolet radiation and radiation of shorter wavelengths can damage biological molecules because these kinds of radiation carry enough energy to break bonds within the molecules. A typical carbon–carbon bond requires 348 kJ/mol to break. What is the longest wavelength of radiation that can break a carbon–carbon bond?

Ultraviolet radiation and radiation of shorter wavelengths can damage biological molecules because they carry enough energy to break bonds within the molecules. A carbon-carbon bond requires 348 kJ/mol to break. What is the longest wavelength of radiation that can still break a carbon-carbon bond?

What is the frequency of a photon emitted when an electron in a hydrogen atom transitions from n = 3 to n = 2? (R_H = 1.097 x 10^7 m^−1)

What is the frequency of light when the energy for a mole of photons is 1.55 x 10^13 J? (Use Planck's constant, h = 6.626 x 10^-34 J·s, and Avogadro's number, 6.022 x 10^23 mol^-1)

What is the frequency of light when the energy of a single photon is 1.48 × 10⁻¹⁵ J? (Use Planck's constant, h = 6.626 × 10⁻³⁴ J·s)

What is the total energy (in kJ) of 1.0 mol of photons with a frequency of 2.75 × 10^14 Hz?