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Ch.5 - Gases

Chapter 5, Problem 65

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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Hi everyone here we have a question telling us that 15 degrees Celsius, 0.76 g of argon gas and 0. g of neon gas are mixed in a 2.3 liter container and it's asking us what are the partial pressure and mole fraction of each gas in the mixture. So first we're going to calculate our molds of argon And that's going to equal 0.76 g times one mole Divided by Aryans Mueller Mass, which is found on the periodic table and is 39.948g. And our g are going to cancel out, giving us 0. moles of Argon. And then we're gonna do the same thing for neon. So our moles of neon Equals 0.59 g times one mole over 20.1797 g. And that equals 0. moles of neon. So our temperature Equals 15°C. And we want to change that to Kelvin. So we're gonna add 273. that equals 288. Kelvin. So our mole fraction of argon is going to equal our moles of argon over the total number of moles, which will be moles of argon plus moles of neon, which equals 0. over 0. plus 0.0 to 9 to four, which equals 0.3941. And to calculate our mole fraction of neon, we can just take one minus our mole fraction of argon because the mole fractions have to equal one. So our mole fraction of neon equals one minus moles of argon. So -0.3941 equals 0.6059. So these are our mole fractions and now we can move on to our partial pressures. So we're going to use the formula PV equals N R. T. So pressure times volume equals number of moles, times our gas constant times our temperature. And we want to solve for pressure. So we're gonna divide both sides by volume. Soapy equals N. R. T. Over. We so our partial pressure of argon equals 0.01902 moles Times 0.08, Times 288.15, divided by 2.3 L, Which equals 0. atmospheres. And now we're gonna do the same for neon. So zero point 0 to 9 to four moles Time, Times 288.15 Kelvin over 2. l equals 0. Atmospheres. So those are our partial pressures. Thank you for watching. Bye
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Textbook Question

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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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

What is the mole fraction of oxygen gas in air (see Table 5.3)? What volume of air contains 10.0 g of oxygen gas at 273 K and 1.00 atm?

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Textbook Question

The hydrogen gas formed in a chemical reaction is collected over water at 30.0 °C at a total pressure of 732 mmHg. What is the partial pressure of the hydrogen gas collected in this way? If the total volume of gas collected is 722 mL, what mass of hydrogen gas is collected?

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Textbook Question

The air in a bicycle tire is bubbled through water and collected at 25 °C. If the total volume of gas collected is 5.45 L at a temperature of 25 °C and a pressure of 745 torr, how many moles of gas were in the bicycle tire?

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