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Heated lithium atoms emit photons of light with an energy of $2.961 \times 10^{-19} {J}$. Calculate the frequency and wavelength of one of these photons. What is the total energy in 1 mole of these photons? What is the color of the emitted light?

$v=4.48 * 10^{-14} \quad \lambda=6.68 * 10^{-8} \quad$ energy per mole $=1.78 * 10^{5}$

Chemistry 101

Chapter 6

Electronic Structure and Periodic Properties of Elements

Electronic Structure

Periodic Table properties

University of Central Florida

Rice University

University of Kentucky

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for this problem. We're told that heated lithium emits photons with an energy of 2.961 times 10 to the negative. 19th Jules perf otan we're asked to do is to calculate the frequency of light emitted from these photons, the wavelength of light as well as the total energy and mole of these photons. And finally, with the color of this light would look like, um so first to calculate the frequency, we're going to use this first equation here to the left. And we're going to solve it in terms of frequency, which is going to equal the given energy, which is again 2.961 times, 10 to the negatives, 19th jewels. And then we're going to divide that by planks constant and the value that we will get out of that is going to be the frequency which in this case is 4.48 times 10 to the 14th hurts. Um, we can then use this frequency value to calculate the corresponding wavelength of this light. We do that using the second equation that I have written here, and we saw that for wavelength, and that's going to be the speed of light. We're going to divide that by the frequency that we just solved for. And that's going to give us a wavelength of 6.68 times 10 to the negative seven meters. Um, the final calculation for this question again is to calculate the energy and a mole of photons att, this given description. So we know that the energy again is 2.961 times 10 to the negative 19 Jules perf Otan s. So we want to know what that value is in terms of mole of photons. We simply multiply it by a big Odgers number, which is gonna be 6.22 times 10 to the 23rd photons in a mole of photons. And the value that we're going to get out of that is 1.78 times 10 to the fifth Jules per mole of the photons emitted by this light. Um, and then finally, they want us to know what the color of this lights going to be. So we consider the color spectrum, and we think about the fact that we're dealing with light that has a wavelength of 668 centimeters. Um, the light that's going to come out of this is going to be visible as red light.

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