In Einstein's photoelectric experiment, the kinetic energy of an electron displaced from a metal by a photon was the difference between the energy of a photon and a threshold energy value for the metal. If you were to perform a similar experiment with cobalt, which has a threshold energy of 8.01 × 10⁻¹⁹ J, and ultraviolet light of wavelength 29.5 nm, what would be the kinetic energy (in J) of the electron displaced?

What is the energy (in J) of a photon with a frequency of 7.23 × 10¹⁴ s⁻¹? (h = 6.626 × 10⁻³⁴ J • s)

The work function (φ) for a metal is the amount of energy needed to eject an electron from the surface of the metal via the photoelectric effect. For nickel φ = 8.25 x 10-19J. Will a photon with a wavelength (λ) of 250.0 nm have enough energy to eject an electron from nickel?  If the speed of an electron in the n = 4 energy level of a hydrogen electron is 2.3 x 106 m/s, what is the de Broglie wavelength of this electron in nanometers (the mass of an electron is 9.10938 x 10-31 kg). Note: 1 ? = 1 ?? ∙?2 An F-15 Strike Eagle weighs in at roughly 32,000 kg fully loaded. If an F-15 Eagle is traveling at 3,017 kilometers per hour, what is the de Broglie wavelength associated with the aircraft at this speed in nanometers?

Determine the energy, in J, of a photon with a wavelength of 351 nm. (h = 6.626 × 10⁻³⁴ J • s and c = 3.00 × 10⁸ m/s)

Determine the energy of a photon, in J, with a wavelength of 294 nm. (h = 6.626 × 10⁻³⁴ J • s and c = 3.00 × 10⁸ m/s) What is the energy (in J) of a mole of photons that have a wavelength of 681 nm? (h = 6.626 × 10⁻³⁴ J • s and c = 3.00 × 10⁸ m/s)

A hydrogen atom absorbs a photon with a wavelength of 1094 nm and causes an electron to make a transition from an unknown n1 to a final n2 = 6.   Part A Calculate frequency of the absorbed photon in units of s-1.       Part B Calculate the energy change in the atom (ΔEatom in J) upon absorption of the photon.     Part C Calculate the value of n1

The minimum energy required to remove an electron from a certain metal is 3.7 x 10– 19 J. If the metal surface is struck by light having a wavelength of 5.00 x 102 nm, what is the kinetic energy of the electron ejected from the metal?

Radiation in the ultraviolet region of the electromagnetic spectrum is quite energetic. It is this radiation that causes dyes to fade and your skin to develop a sunburn. If you are bombarded with 1.00 mol of photons with a wavelength of 320. nm, what amount of energy, in kilojoules per mole of photons, are you being subjected to? Energy = kJ/mol

Determine the energy, in J, of a photon with a wavelength of 327 nm. (h = 6.626 × 10⁻³⁴ J • s and c = 3.00 × 10⁸ m/s)

What is the frequency of a photon if the energy is 7.33 × 10⁻¹⁹ J? (h = 6.626 × 10⁻³⁴ J • s)