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Ch.10 - Gases

Chapter 10, Problem 81b

(b) Calculate the rms speed of NF3 molecules at 25 °C.

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Hey everyone. So here we asked. The root mean square velocities of chlorine gas, argon gas, hydro biotic acid. And the temperature is 300 Kelvin. So the root mean square velocity Visit to the Square Root of three R. T. About about a Mueller mass. So far our value have 8. jaws about about moles tom's kelvin. And we know that jules executive kilograms, thomas meter squared about by seconds squared. So far our value of 8. kilograms times meters squared. About about malls times kelvin times seconds squared. Look at the root mean square velocity of chlorine gas, We're gonna get three Times 8. telegrams. I'm his meter squared, invited by malls times Calvin second squared Times 300 Kelvin by the molar mass. It's gonna be too It was a massive chlorine which is .453. This give us 70 .906g. But this has to be in kilograms. They're gonna have 70 .906g In 1000 g of one kg And it will give us 0.0709 telegrams 0.0709 kilograms per mole solar mass. This give us 324 0.87 Minutes for a 2nd. The root mean square velocity of argon gas. We're gonna have the square root three 8.314 milligrams. House meter squared. What about mose name's Calvin? I'm second squared Times 300 Kelvin by the molar mass. And this is 39.948. We need to convert two kg 1000 g in one kg. And this will give us 0.39 telegrams, 0.39 948 kilograms per mole. The molar mass This gave us 0.79. Meet us for a second at the root mean squared velocity of hydro biotic acid. It's going to be the square root three Times 8.314 kilograms times meters squared. What about moles, thomas, kelvin, second squared Times 300 Kelvin by by the molar mass hydro biotic acid. It's gonna be a mass of hydrogen which is 1.008 g. That's a massive iodine. 126 .904. Nice to give us 127 .912 grams. We need to convert two kg 1000 g of one kg. This will give us 0.12 telegrams, 0.12 7912 kilograms per mold the molar mass. And this will give us 241 0.86. Meet us for a second. Thanks for watching my video and I hope it was helpful
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Textbook Question

Suppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (a) number of molecules?

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Textbook Question

Suppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (b) density?

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Textbook Question

Suppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (c) average kinetic energy of the molecules?

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Textbook Question

(c) Calculate the most probable speed of an ozone molecule in the stratosphere, where the temperature is 270 K.

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Textbook Question

Which one or more of the following statements are true? (a) O2 will effuse faster than Cl2. (b) Effusion and diffusion are different names for the same process. (c) Perfume molecules travel to your nose by the process of effusion. (d) The higher the density of a gas, the shorter the mean free path.

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Textbook Question

At constant pressure, the mean free path 1l2 of a gas molecule is directly proportional to temperature. At constant temperature, l is inversely proportional to pressure. If you compare two different gas molecules at the same temperature and pressure, l is inversely proportional to the square of the diameter of the gas molecules. Put these facts together to create a formula for the mean free path of a gas molecule with a proportionality constant (call it Rmfp, like the ideal-gas constant) and define units for Rmfp.

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