Photovoltaic cells convert solar energy into electricity. Calculate the wavelength of light (in nm) required for tantalum ( =6.81× 10-19 J) to emit anelectron. Then determine whether or not tantalum could be used to generate electricity from the sun. Assume that most of the electromagneticenergy from the sun is in the visible region near 500 nm. The wavelength of light (in nm) required for tantalum ( =6.81 × 10-19 J) to emit an electron:nmCould tantalum be used to generate electricity from the sun?Choose one:O Yes, the threshold wavelength is larger than the wavelength of the sun so electricity is generated.O No, the threshold wavelength is larger than the wavelength of the sun so electricity will not be generated.No, the threshold wavelength is lower than the wavelength of the sun so electricity will not be generated.O Yes, the threshold wavelength is lower than the wavelength of the sun so electricity will be generated.

Answered: Image /qna-images/answer/c4ee9c5e-bd38-4d47-9f25-0770615d6778.jpg

Answered: The wavelength of light (in nm)…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 36QRT

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(a) Which color in the visible spectrum has the highest frequency? Which has the lowest frequency? (b) Is the wavelength of the radiation used in a microwave oven (2.45 GHz) longer or shorter than that from your favorite FM radio station (for example, 91.7 MHz)? (c) Are the wavelengths of x-rays longer or shorter than those of ultraviolet light? (d) Calculate the frequency of green light with a wavelength of 510. nm.
A hydrogen atom in the ground stale absorbs a photon whose wavelength is 95.0 nm. The resulting excited atom then emits a photon of 1282 nm. What are the regions of the electromagnetic spectrum for the radiations involved in these transitions? What is the principal quantum number of the final state resulting from the emission from the excited atom?
Traffic signals are often now made of LEDs (light-emitting diodes). Amber and green ones are pictured here. (a) The light from an amber signal has a wave-length of 595 nm, and that from a green signal has a wavelength of 500 nm. Which has the higher frequency? (b) Calculate the frequency of amber light.
An FM radio station found at 103.1 on the FM dial broadcasts at a frequency of 1.031188s1 (103.1 MHz). What is the wavelength of these radio waves in meters?
An energy of 3.3 1019 J/atom is required to cause a cesium atom on a metal surface to lose an electron. Calculate the longest possible wavelength of light that can ionize a cesium atom. In what region of the electromagnetic spectrum is that radiation found?
Warm objects emit electromagnetic radiation in the infrared region. Heat lamps employ this principle to generate infrared radiation. Water absorbs infrared radiation with wavelengths near 2.80 m. Suppose this radiation is absorbed by the water and converted to heat. A 1.00-L sample of water absorbs infrared radiation, and its temperature increases from 20.0C to 30.0C. How many photons of this radiation are used to heat the water?
A particular microwave oven delivers 750 watts. (A watt is a unit of power, which is the joules of energy delivered, or used, per second.) If the oven uses microwave radiation of wavelength 12.6 cm, how many photons of this radiation are required to heat 1.00 g of water 1.00C, assuming that all of the photons are absorbed?
Which of the following sets of quantum numbers correctly represents a 4p orbital? (a) n = 4, = 0, m = 1 (b) n = 4, = 1, m = 0 (c) n = 4, = 2, m = 1 (d) n = 4, = 1, m =2

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