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Chapter 8: Problem 11

Use Planck's equation (8.3) to determine (a) the energy, in joules per photon, of radiation of frequency $7.39 \times 10^{15} \mathrm{s}^{-1}$ (b) the energy, in kilojoules per mole, of radiation of frequency $1.97 \times 10^{14} \mathrm{s}^{-1}$

Short Answer

Expert verified
a) The energy of radiation per photon is around \(4.9 \times 10^{-18}\) Joules. b) The energy of radiation per mole is around \(78.1\) Kilojoules.

Step by step solution

01

Calculating photon energy (part a)

Using the Planck's equation \(E = h\times v\), and substituting Planck's constant \(h\) as \(6.626 \times10^{-34}\) Js and frequency \(v\) as \(7.39 \times 10^{15}\) s^(-1), we can calculate the energy \(E\).
02

Convert joules to kilojoules (part b)

Still using the Planck's equation, we substitute Planck's constant and frequency \(v\) as \(1.97 \times 10^{14}\) s^(-1) to find the energy per photon. Then we multiply this value by Avogadro's number, \(6.022 \times 10^{23}\) to find the energy per mole, and divide by \(10^{3}\) to convert from Joules to Kilojoules.

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