Giancoli's Physics: Principles with Applications, 7th Edition

13

Temperature and Kinetic Theory

Change chapter13-1: Atomic Theory

13-2: Temperature and Thermometers

13-4: Thermal Expansion

13-5: Gas Laws; Absolute Temperature

13-6 and 13-7: Ideal Gas Law

13-8: Ideal Gas Law in Terms of Molecules; Avogadro's Number

13-9: Molecular Interpretation of Temperature

13-11: Real Gases; Phase Changes

13-12: Vapor Pressure and Humidity

13-13: Diffusion

Question by Giancoli, Douglas C., Physics: Principles with Applications, 7th Ed., ©2014, Reprinted by permission of Pearson Education Inc., New York.

Problem 51

Q

A

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VIDEO TRANSCRIPT

This is Giancoli Answers with Mr. Dychko. *V rms1* is going to be square root of 3 times Boltzmann's constant times temperature divided by the molecular mass of the first atom. And this *M* is usually a lowercase *m* but I'm writing a capital *M* because that's what they did in that question here. And this is the mass of a single molecule which is molecular mass. So, *V rms2* is going to be square root of 3 *K T* over molecular mass of the second type of stuff. So, a *V rms2* divided by *V rms1* it's going to be square root 3 *K T* over *M2*, that's V rms2. And when dividing by *V rms1* I'm going to instead multiply by its reciprocal so that we can see more easily how things cancel. And we have 3 *K T* here and square root of 3 *K T* here, they cancel and we're left with square root *M1* over *M2*. So, the speed, rms, of the second thing divided by the rms speed of the first type of material is going to be the square root of *M1* over *M2*. So, that's the inverse ratio of the molecular mass square rooted.

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