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Exam 5: Gases and the Kinetic-Molecular Theory

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Question 1

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"The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of moles" is a statement of __________________ Law.

A) Charles's
B) Boyle's
C) Amontons's
D) Avogadro's
E) Gay-Lussac's

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Question 2

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Arrange the following gases in order of increasing rate of effusion: C₂H₆, Ar, HCl, PH₃

A) Ar < HCl <PH₃ < C₂H₆
B) C₂H₆ < PH₃ < HCl < Ar
C) Ar < PH₃ < C₂H₆ < HCl
D) C₂H₆ < HCl < PH₃ < Ar
E) Ar <PH₃ < HCl < C₂H₆

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Question 3

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A 750-mL sample of hydrogen exerts a pressure of 822 torr at 325 K. What pressure does it exert if the temperature is raised to 475 K at constant volume?

For an ideal gas, a plot of PV/nRT versus P gives a straight line with a positive slope.

State Charles's Law and illustrate it with a graph, using standard x-y coordinate axes. Be sure to label the axes unambiguously with the correct gas variables.

If 0.750 L of argon at 1.50 atm and 177 $\degree$ C and 0.235 L of sulfur dioxide at 95.0 kPa and 63.0 $\degree$ C are added to a 1.00-L flask and the flask's temperature is adjusted to 25.0 $\degree$ C, what is the resulting pressure in the flask?

Which of the lines on the figure below is the best representation of the relationship between the volume and the number of moles of a gas, measured at constant temperature and pressure?

Methane, CH₄(g) , reacts with steam to give synthesis gas, a mixture of carbon monoxide and hydrogen, which is used as starting material for the synthesis of a number of organic and inorganic compounds. CH₄(g) + H₂O(g) $\rightarrow$ CO(g) + H₂(g) [unbalanced] What mass of hydrogen is formed if 275 L of methane (measured at STP) is converted to synthesis gas?

Calculate the root-mean-square speed of methane, CH₄ (g) , at 78 $\degree$ C.

The most probable speed of an oxygen molecule in the gas phase at room temperature is 450 m/s. The root-mean-square speed (u_rms) is therefore

An unknown liquid is vaporized in a 273-mL flask by immersion in a water bath at 99 $\degree$ C. The barometric pressure is 753 torr. If the mass of the vapor retained in the flask is 1.362 g, what is its molar mass?

A sample of methane gas, CH₄(g) , occupies a volume of 60.3 L at a pressure of 469 torr and a temperature of 29.3 $\degree$ C. What would be its temperature at a pressure of 243 torr and volume of 60.3 L?

Starting from the Ideal Gas Equation, derive an equation corresponding to Charles's Law, stating all important assumptions or conditions.

A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37.0 $\degree$ C. How many moles of nitrogen are in the container?

A flask containing helium gas is connected to an open-ended mercury manometer. The open end is exposed to the atmosphere, where the prevailing pressure is 752 torr. The mercury level in the open arm is 26 mm above that in the arm connected to the flask of helium. What is the helium pressure, in torr?

A flask containing neon gas is connected to an open-ended mercury manometer. The open end is exposed to the atmosphere, where the prevailing pressure is 745 torr. The mercury level in the open arm is 50. mm below that in the arm connected to the flask of neon. What is the neon pressure, in torr?

At a temperature of absolute zero, the volume of an ideal gas is zero.

"The pressure of an ideal gas is directly proportional to its absolute temperature at constant volume and number of moles" is a statement of ________________ Law.

Mineral oil can be used in place of mercury in manometers when small pressure changes are to be measured. What is the pressure of an oxygen sample in mm of mineral oil if its pressure is 28.5 mm Hg? (d of mineral oil = 0.88 g/mL; d of Hg = 13.5 g/mL)

Mercury is 13.6 times as dense as liquid water. What would be the reading of a water-filled barometer at normal atmospheric pressure, 760. mmHg?