Given:
lambda = 550 nm = 5.50*10^-7 m
use:
E = h*c/lambda
=(6.626*10^-34 J.s)*(3.0*10^8 m/s)/(5.5*10^-7 m)
= 3.614*10^-19 J
Answer: 3.61*10^-19 J
9. Determine the energy of an electromagnetic radiation of 550 nm wavelength.
For electromagnetic radiation with a wavelength of 213.5 nm: (a) What is the frequency of the radiation (in s-1)? (b) What is the energy (in J) of one photon of the radiation? (c) What is the energy (in kJ) of one mole of photons of the radiation?
14. Electromagnetic radiation human eye. How many photo ectromagnetic radiation with a wavelength of 522 nm appears as green light to the n eye. How many photons are produced in each pulse by a laser that emits 1.3x10 J of energy in a pulse of light at this wavelength.
s) Electromagnetic radiation with a wavelength of 575 nm appears as yellow light to the human eye. Calculate the energy of one photon of this light. A) 3.46 x10-19 B) 3.46 x10-28 J C) 1.14 x 10-22 J D) 1.14 x 10-31J E) 2.34x 1018J 18)
of its kinetic energy to its fest citib . An experiment shows that when electromagnetic radiation of wavelength 270 nm falls on an aluminum surface, photoelectrons are emitted. The most energetic of these are stopped by a potential difference of 0.406 volts. Use this information to calculate the work function of aluminum in electron volts. of its kinetic energy to its fest citib . An experiment shows that when electromagnetic radiation of wavelength 270 nm falls on an aluminum surface,...
When electromagnetic radiation with a wavelength of 326.0 nm is directed at the surface of a certain metal, electrons are ejected from the surface with a de Broglie wavelength of 9.65 Å. Calculate the work function for the metal in kJ/mole of e ejected. 1 Å (angstrom) = 1x10 meters kJ/mol e Check
7 Find the energy of the photons for each of the following types of electromagnetic radiation: radio wave of wavelength 80.0 cm; violet light of wavelength 390 nm; X-ray of wavelength o.250 nm
Determine the frequency and energy for light with a wavelength of 697.7 nm. kJ/mol What is the color of light with a wavelength of 697.7 nm? Refer to the electromagnetic spectrum as needed. Determine the wavelength and energy for light with a frequency of 5.809 x 101 - kJ/mol What is the color of light with a frequency of 5.809 x 10' +'? Refer to the electromagnetic spectrum as needed, What is the color of light with a frequency of...
Consider the relationship between the energy of electromagnetic radiation and its wavelength. What will happen if the energy decreases? The wavelength will remain the same. The wavelength will decrease. The wavelength will increase. What will happen if the wavelength decreases? The energy will decrease. The energy will remain the same. The energy will increase.
Calculate the energy per photon and the energy per mole of photons for radiation of wavelength (i) 600 nm (red), (ii) 550 nm (yellow), (iii) 400 nm (blue).
Electromagnetic radiation of wavelength 96.4 nm was projected on a zinc plate with a 6.01×10-19 J of work function. Calculate the kinetic energy of an emitted electron. a. -6.01×10-19 J b. 1.46×10-18 J c. 28.9 J d. 2.66×10-18 J e. 4.69×1048 J