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Ch.10 - Gases
All textbooksBrown 14th EditionCh.10 - GasesProblem 111
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Chapter 10, Problem 111

A glass vessel fitted with a stopcock valve has a mass of 337.428 g when evacuated. When filled with Ar, it has a mass of 339.854 g. When evacuated and refilled with a mixture of Ne and Ar, under the same conditions of temperature and pressure, it has a mass of 339.076 g. What is the mole percent of Ne in the gas mixture?

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1
Calculate the mass of Ar in the vessel by subtracting the mass of the evacuated vessel from the mass of the vessel filled with Ar: 339.854 g - 337.428 g.
Calculate the mass of the Ne and Ar mixture by subtracting the mass of the evacuated vessel from the mass of the vessel filled with the mixture: 339.076 g - 337.428 g.
Determine the mass of Ne in the mixture by subtracting the mass of Ar (from step 1) from the mass of the Ne and Ar mixture (from step 2).
Use the molar masses of Ne (20.18 g/mol) and Ar (39.95 g/mol) to convert the masses of Ne and Ar to moles.
Calculate the mole percent of Ne in the mixture by dividing the moles of Ne by the total moles of Ne and Ar, then multiply by 100 to get the percentage.
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Textbook Question
An ideal gas at a pressure of 152 kPa is contained in a bulb of unknown volume. A stopcock is used to connect this bulb with a previously evacuated bulb that has a volume of 0.800 L as shown here. When the stopcock is opened, the gas expands into the empty bulb. If the temperature is held constant during this process and the final pressure is 92.66 kPa, what is the volume of the bulb that was originally filled with gas?

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Textbook Question

The density of a gas of unknown molar mass was measured as a function of pressure at 0 C, as in the table that follows. (a) Determine a precise molar mass for the gas. [Hint: Graph d>P versus P.]

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The density of a gas of unknown molar mass was measured as a function of pressure at 0 C, as in the table that follows. (b) Why is d>P not a constant as a function of pressure?

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You have a sample of gas at 0 C. You wish to increase the rms speed by a factor of 3. To what temperature should the gas be heated?
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Textbook Question

Consider the following gases, all at STP: Ne, SF6, N2, CH4. (a) Which gas is most likely to depart from the assumption of the kinetic-molecular theory that says there are no attractive or repulsive forces between molecules?

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Textbook Question

Consider the following gases, all at STP: Ne, SF6, N2, CH4. (d) Which one has the highest total molecular volume relative to the space occupied by the gas?

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