An ultraviolet photon with a wavelength of 320 nm strikes a metal surface. The emitted electron has a kinetic energy of 3.0 x 10^-2 eV. What is the binding energy of the electron in kJ/mol? 1 electron volt (eV) = 1.602 x 10^-19 J.

Assuming total absorption of the light by the sample, what is the maximum amount (in moles) of CH3X that breaks apart when a cuvette containing a solution of CH3X is irradiated with 280-nm light with a power of 885 mW for 10.0 minutes, given that the quantum yield for the reaction CH3X → CH3 + X is f = 0.24?

A student is studying the photodissociation (dissociation with light) of I2 into 2I. When a sample of I2 is irradiated with a power of 255 mW at 590 nm for 35 seconds, 0.0256 mmol of I forms. Assuming complete absorption of the incident radiation, what is the quantum yield, f, of the reaction? (See Problem 93 for definition of quantum yield.)

The energy required to dislodge electrons from sodium metal via the photoelectric effect is 275 kJ/mol. What wavelength (in nm) of light has sufficient energy per photon to dislodge an electron from the surface of sodium?

Which best describes the photoelectric effect?

Which of the following is true about the photoelectric effect?

Which type of electromagnetic radiation will cause the greatest number of electrons to be ejected from zinc metal with a work function of 350 kJ/mol? (LO 5.4, 5.5)(a) Dim light with a wavelength of 320 nm (b) Dim light with a wavelength of 360 nm (c) Bright light with a wavelength of 360 nm (d) Bright light with a wavelength of 375 nm

Einstein's 1905 paper on the photoelectric effect was thefirst important application of Planck's quantum hypothesis.Describe Planck's original hypothesis, and explain howEinstein made use of it in his theory of the photoelectriceffect.