9. Quantum Mechanics

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm. Use the formula E = hc/λ, where h = 6.626 x 10^-34 J·s and c = 3.00 x 10^8 m/s.

Determine the energy, in joules per photon, of radiation with a frequency of 8.52 × 10^15 s⁻¹.

What is the minimum frequency of light required to remove an electron from a titanium metal sample, given that the binding energy of titanium is 3.14 × 10^3 kJ/mol?

Green light has a frequency of about 6.00 × 10^14 s^-1. What is the energy of a photon of green light?

How many photons are contained in a burst of yellow light (589 nm) from a sodium lamp that contains 609 kJ of energy?

How many photons are contained in a flash of green light (525 nm) that contains 189 kJ of energy?

How much energy (in joules) is contained in 1.00 mole of 552 nm photons?

How much energy (in kJ) do 3.0 moles of photons, all with a wavelength of 655 nm, contain?

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 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 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)