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

Calculate the energy of the red light emitted by a neon atom with a wavelength of 680 nm. Use the formula E = hc/λ, where h is Planck's constant (6.626 x 10^-34 J·s) and c is the speed of light (3.00 x 10^8 m/s).

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?

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?