/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 20 It is possible to convert radian... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 6: Problem 20

It is possible to convert radiant energy into electrical energy using photovoltaic cells. Assuming equal efficiency of conversion, would infrared or ultraviolet radiation yield more electrical energy on a per-photon basis?

Short Answer

Expert verified
On a per-photon basis, ultraviolet radiation would yield more electrical energy compared to infrared radiation, assuming equal efficiency of conversion in photovoltaic cells. This is because the energy of a photon is directly proportional to its frequency and the frequency of ultraviolet radiation is higher than that of infrared radiation.

Step by step solution

01

Understanding electromagnetic spectrum and radiant energy

The electromagnetic spectrum contains various types of waves, including infrared and ultraviolet radiation. Radiant energy is the energy carried by electromagnetic waves. The radiant energy carried by a wave is directly proportional to its frequency.
02

Recall the energy of a photon formula

To determine the energy of a photon, we use the following formula: \(E = h\nu\) where \(E\) represents the energy of a photon, \(h\) is the Planck's constant (\(6.63 \times 10^{-34} Js\)), and \(\nu\) is the frequency of the electromagnetic wave.
03

Understanding the position of infrared and ultraviolet radiation in the electromagnetic spectrum

In the electromagnetic spectrum, infrared radiation has a lower frequency compared to visible light, while ultraviolet radiation has a higher frequency compared to visible light. This means that the frequency of ultraviolet radiation is higher than the frequency of infrared radiation.
04

Comparing the energy of infrared and ultraviolet photons

Since the energy of a photon is directly proportional to its frequency and the frequency of ultraviolet radiation is higher compared to infrared radiation, it follows that the energy per photon of ultraviolet radiation is greater than the energy per photon of infrared radiation.
05

Conclusion

On a per-photon basis, ultraviolet radiation would yield more electrical energy compared to infrared radiation, assuming equal efficiency of conversion in photovoltaic cells.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

The energy from radiation can be used to cause the rupture of chemical bonds. A minimum energy of \(941 \mathrm{~kJ} / \mathrm{mol}\) is required to break the nitrogen-nitrogen bond in \(\mathrm{N}_{2}\). What is the longest wavelength of radiation that possesses the necessary energy to break the bond? What type of electromagnetic radiation is this?

The first 25 years of the twentieth century were momentous for the rapid pace of change in scientists' understanding of the nature of matter. (a) How did Rutherford's experiments on the scattering of \(\alpha\) particles by a gold foil set the stage for Bohr's theory of the hydrogen atom? (b) In what ways is de Broglie's hypothesis, as it applies to electrons, consistent with J. J. Thomson's conclusion that the electron has mass? In what sense is it consistent with proposals preceding Thomson's work that the cathode rays are a wave phenomenon?

(a) A red laser pointer emits light with a wavelength of \(650 \mathrm{nm}\). What is the frequency of this light? (b) What is the energy of one of these photons? (c) The laser pointer emits light because electrons in the material are excited (by a battery) from their ground state to an upper excited state. When the electrons return to the ground state, they lose the excess energy in the form of \(650 \mathrm{nm}\) photons. What is the energy gap between the ground state and excited state in the laser material?

Which of the quantum numbers governs (a) the shape of an orbital, (b) the energy of an orbital, (c) the spin properties of the electron, \((\) d) the spatial orientation of the orbital?

The series of emission lines of the hydrogen atom for which \(n_{f}=3\) is called the Paschen series. (a) Determine the region of the electromagnetic spectrum in which the lines of the Paschen series are observed. (b) Calculate the wavelengths of the first three lines in the Paschen series-those for which \(n_{i}=4,5,\) and 6
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.