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What is the ratio of the average kinetic energy of a $SO_{2}$ molecule to that of an $\mathrm{O}_{2}$ molecule in a mixture of two gases? What is the ratio of the root mean square speeds, $u_{\mathrm{rms}},$ of the two gases?
$1 : 1$$0.707 : 1$
01:28
Aadit S.
Chemistry 101
Chapter 9
Gases
Drexel University
University of Maryland - University College
Brown University
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so continuing on with the molecular Speedo the root mean square velocity. So those equations air expressed on this page here in these expressions, if you'd like to refer back to them in the previous podcast. So as the molecular speed of the brute means Squire velocity of a particles of gas, a continent temperatures and vastly proportional to the mass, we see that you root means square is proportional to one over square roots. So if we have two classes, for example, you root mean square a bye bye, you root mean square B. We have roots M B over M A. So, according to the kinetic molecular theories, the average kinetic and achieve the two glasses, it's the same at the same temperature. So the average kinetic energy of the two gasses after two and so too will not change, and therefore the ratio of average kinetic energies of the two will be a 1 to 1. So just the last portion of the podcasters. So the molecular mass of a so too, is listed on the photo to and so we have argue it means square for eso to try to buy you. It means square for 02 is equal to square root. 32 grams per mols, minus one divided by 64 g per mole to the minus. What this gives us a value off not 0.707 in the ratio of the root, mean square velocities will be no 0.701 21 707 to 1.
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