A gas mixture with a total pressure of 745 mmHg contains each of the following gases at the indicated partial pressures: CO 2 , 125 mmHg; Ar, 214 mmHg; and O 2 , 187 mmHg. The mixture also contains helium gas. What is the partial pressure of the helium gas? What mass of helium gas is present in a 12.0-L sample of this mixture at 273 K?

Hey everyone. So you were asked catholic, the pressure pressure of xenon in the gas mixture, The total pressure of 7 - 84 mm of Mercury. And the partial pressures of the other gasses are hydrogen gas, which is 56 km. and Mercury Um is 198 million. Museum records. Natural Gas is 263 mm of Mercury. When we asked consider an 8l sample of the mixture At 298 Kelvin and to calculate the mass of the xenon gas. So for the total pressure with the partial pressure of the xenon gas plus the partial pressure of hydrogen gas, the partial pressure of helium, that's the partial pressure of nitrogen gas. We plug in the values we have 784 millimeters of mercury. Even to the partial pressure of xenon gas was 56 bellamy's a mercury Plus 1 98. Mail me as a mercury passenger 63. Tell me as a mercury And then we have 7-84. Tell me some rectory into the partial pressure of xenon gas. That's 517 filmmakers of mercury. Sophie's attract both sides by 517. Killing me some record, we get that the partial pressure of xenon gas, It's 267. Film use of mercury. So now we need to use the ideal gas law equation to find the mass of Xenon. This is P V N R. T. We're in is the number of moles, which is equal to the mass by, by the Mueller mass plug this in for n We're gonna get PV. He goes M. R. T. What about Mueller mass? Now if you rearrange this is all for em gonna get em equals PV some similar mass. What about R. T. For the pressure Up 267 filmmakers of mercury For the volume. We have eight L. We're looking for the mass for art. 0.08 21. There's some atmosphere name's kelvin. And the temperature is 298 Calvin for the Mueller mass of xenon, That 1-31 .29g. So now we need to convert our pressure from millimeters of mercury to atmosphere. We have 267 millimeters of mercury. We have 760 millimeters of mercury in one atmosphere And this will give us 0.351 atmosphere. So now if you plug in advice into the equation we're gonna get em Equals 0.351 atmosphere times eight Leaders Times 0.29 grams per remote Divided by 0.08 26. Later sounds atmosphere Calvin Comes 298 kelvin. So for the mass we're gonna get 15.1 g. Thanks for watching my video and I hope it was helpful

Ch.6 - Gases

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Problem 62

Chapter 6, Problem 62

A gas mixture with a total pressure of 745 mmHg contains each of the following gases at the indicated partial pressures: CO₂, 125 mmHg; Ar, 214 mmHg; and O₂, 187 mmHg. The mixture also contains helium gas. What is the partial pressure of the helium gas? What mass of helium gas is present in a 12.0-L sample of this mixture at 273 K?

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Identify the total pressure of the gas mixture, which is given as 745 mmHg.

List the partial pressures of the known gases: CO2 is 125 mmHg, Ar is 214 mmHg, and O2 is 187 mmHg.

Use Dalton's Law of Partial Pressures, which states that the total pressure is the sum of the partial pressures of all gases in the mixture. Set up the equation: P_total = P_CO2 + P_Ar + P_O2 + P_He.

Rearrange the equation to solve for the partial pressure of helium (P_He): P_He = P_total - (P_CO2 + P_Ar + P_O2).

To find the mass of helium, use the ideal gas law: PV = nRT. Solve for n (moles of He) using the partial pressure of He, the volume (12.0 L), and the temperature (273 K). Then, convert moles to grams using the molar mass of helium (4.00 g/mol).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Dalton's Law of Partial Pressures

Dalton's Law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas. This principle allows us to calculate the partial pressure of an unknown gas in a mixture by subtracting the known partial pressures from the total pressure.

Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for calculating the mass of a gas when its volume, temperature, and pressure are known, as it allows us to determine the number of moles and subsequently convert to mass using the molar mass.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the number of moles of a gas and its mass. Knowing the molar mass of helium (approximately 4.00 g/mol) enables us to calculate the mass of helium present in the gas mixture once we determine the number of moles using the Ideal Gas Law.

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Molar Mass Concept

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Textbook Question

A 1.20-g sample of dry ice is added to a 755 mL flask containing nitrogen gas at a temperature of 25.0 °C and a pressure of 725 mmHg. The dry ice sublimes (converts from solid to gas), and the mixture returns to 25.0 °C. What is the total pressure in the flask?

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Textbook Question

A 275-mL flask contains pure helium at a pressure of 752 torr. A second flask with a volume of 475 mL contains pure argon at a pressure of 722 torr. If we connect the two flasks through a stopcock and we open the stopcock, what is the partial pressure of argon?

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Textbook Question

A gas mixture contains 1.25 g N₂ and 0.85 g O₂ in a 1.55 L container at 18 °C. Calculate the mole fraction and partial pressure of each component in the gas mixture.

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