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A gas mixture contains each of the following gases at theindicated partial pressures: N2N2,239 torr ; O2O2, 133 torr ; and HeHe,107 torr.What mass of each gas is pr...

Question

A gas mixture contains each of the following gases at theindicated partial pressures: N2N2,239 torr ; O2O2, 133 torr ; and HeHe,107 torr.What mass of each gas is present in a 1.45 −L−L sampleof this mixture at 25.0 ∘C∘C? Enter your answers numerically separated by commas.mN2,mO2,mHe =

A gas mixture contains each of the following gases at the indicated partial pressures: N2N2, 239 torr ; O2O2, 133 torr ; and HeHe, 107 torr. What mass of each gas is present in a 1.45 −L−L sample of this mixture at 25.0 ∘C∘C? Enter your answers numerically separated by commas. mN2,mO2,mHe =



Answers

A gas mixture contains each of these gases at the indicated partial pressures: N2, 215 torr; O2, 102 torr; and He, 117 torr. What is the total pressure of the mixture? What mass of each gas is present in a 1.35-L sample of this mixture at 25.0 C?

This question is testing our understanding to partial pressure. So the total pressure equals to the partial. The total pressure equals to the some off the partial pressure of all the components. So the total pressure in this condition you close to the partial pressure off natural oxygen and aunt he on helium gas, which is 400 under 30 under 34 tours, also eat according to ideal gas loss. Peavey was to an arty on in this condition. If we calculate if we calculate the PS, the total pressure on this question tells us temperature is 25 Celsius degrees. The volume is well 101.23 five liters. Based on there's the equation, we can calculate the amount off, I guess is the amount of gas is C moc in total. So the, um, the be and the most off nitrogen, oxygen and helium gases, the ratio it equals to their partial. They're they're partial pressure. The ratio of their partial pressure in this case is 215 over 100 under to over 117 on the total number off. The total number you most is is the same as well, we calculate here, which is unwto tal so we can calculate the for Each gas is on under the mass of each gases. We can calculate that. So the must off National Jin, Is there a point of 437 grams? The mass of oxygen is Nero pointed to several 237 grams And the muscle helium is there a 2370.34 grams?

This question tells us that a gas make sure contains each of these gases at their indicated partial pressures and asked us for the total pressure of the mixture. So here we have nitrogen at 2 17 tour oxygen at one of six tour and helium at 2 48 tour. So to find total pressure from partial pressures, um P total this is Dolphins law. P total equals the pressure of guests. A plus, the pressure of CIA puts pressure, Cassie and so on until you've get counted for every gas in the mixture. So here are P total will be the pressure of the nitrogen gas, plus the pressure of the oxygen gas, plus the pressure of the healing guests. So that will be P total will be to 17 tour plus one of six poor plus 2 48 tour. So our P total is going to be 5 71 tour

This is a fairly easy calculation. Dalton's law of partial pressure states that the total pressure is the sum of all the partial pressures. So what we need to do is some up the partial pressures in units of tour in order to get the total pressure of 765 tour for the mixture.

Hi There in Probleble # 81. We have a mixture of three different gases and we are given the pressure of each of those gases. That is known as the partial pressure of each gas. And the question wants to know the total pressure in the mixture. So we have to remember Dalton's off partial pressure. Dalton's off partial pressure says the total pressure Is equal to the pressure of gas, one plus the pressure of gas too. And so on. Until we find the sum of all of the gases in the sample, the pressure for all the gases. So in this we just have three gases. We have nitrogen That has a pressure of 315 tour or a partial pressure. We have oxygen that has a partial pressure of 275 tour and we have Are gone. That has a partial pressure of 285 tour. Yes. So adding these all together each of these total each of these partial pressures. We'll add them together to get the total pressure of the sample. And that is going to be 875 tour. Yeah. The second part of this question asks about the mole fraction of the oxygen. Remember this to 75. Here was the oxygen. So to find the mole fraction of the oxygen we take the pressure of the oxygen. This is an equation from the unit for us. We can take the pressure of the oxygen divided by the total pressure. Mhm. So the pressure of the oxygen was 275 tour. The total pressure we calculated to be 875 tour. Therefore the mole fraction of the oxygen is going to be point 314 Okay. Okay. And that is the second, Yeah. Mhm. Okay. Part of the answer to this question. So we have the total pressure of the sample and the mole fraction of the oxygen. Yeah. Mhm.


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