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)

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

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 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?

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

Convert 4.5 x 10^-15 J/photon to wavelength in nm. Which of the following is the correct wavelength?