Logout Open In App
Open In App
Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

Indicate whether energy is emitted or absorbed when the following electronic transitions occur in hydrogen: (a) from \(n=2\) to \(n=6,\) (b) from an orbit of radius \(4.76 \AA\) to one of radius \(0.529 \AA,(\mathrm{c})\) from the \(n=6\) to the \(n=9\) state.

The following electron configurations represent excited states. Identify the element, and write its ground-state condensed electron configuration. (a) \(1 s^{2} 2 s^{2} 3 p^{2} 4 p^{1},\) (b) \([\mathrm{Ar}] 3 d^{10} 4 s^{1} 4 p^{4} 5 s^{1}\), (c) \([\mathrm{Kr}] 4 d^{6} 5 s^{2} 5 p^{1}\) (a) Determine which elements emit radiation in the visible part of the spectrum. (b) Which element emits photons of highest energy? Of lowest energy? (c) When burned, a sample of an unknown substance is found to emit light of frequency \(6.59 \times 10^{14} \mathrm{~s}^{-1}\). Which of these elements is probably in the sample?

The electron microscope has been widely used to obtain highly magnified images of biological and other types of materials. When an electron is accelerated through a particular potential field, it attains a speed of \(8.95 \times 10^{6} \mathrm{~m} / \mathrm{s}\). What is the characteristic wavelength of this electron? Is the wavelength comparable to the size of atoms?

Explain how the existence of line spectra is consistent with Bohr's theory of quantized energies for the electron in the hydrogen atom.

Sketch the shape and orientation of the following types of orbitals: \((\mathbf{a}) p_{x},(\mathbf{b}) d_{z^{2}},(\mathbf{c}) d_{x^{2}-\gamma^{2}}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Chemical Analysis

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic 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.

Sign-up for free