Ch.10 - Gases

Problem 13

Chapter 10, Problem 13

Which of the following statements is false? (a) Gases are far less dense than liquids. (b) Gases are far more compressible than liquids. (c) Because liquid water and liquid carbon tetrachloride do not mix, neither do their vapors. (d) The volume occupied by a gas is determined by the volume of its container.

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Let's analyze each statement one by one to determine which one is false.

(a) Gases are far less dense than liquids. This statement is true. Gases have a much lower density than liquids because their particles are spread out and not as closely packed together.

(b) Gases are far more compressible than liquids. This statement is also true. Gases are more compressible because their particles are not as closely packed together, allowing them to be squeezed into a smaller volume.

(c) Because liquid water and liquid carbon tetrachloride do not mix, neither do their vapors. This statement is false. The fact that two liquids do not mix does not necessarily mean their vapors will not mix. In the gaseous state, the particles are much more spread out and can easily intermingle, regardless of whether or not they mix in the liquid state.

(d) The volume occupied by a gas is determined by the volume of its container. This statement is true. Gases will expand to fill the volume of their container, regardless of the size of the container.

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Key Concepts

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

Density of Gases vs. Liquids

Density is a measure of mass per unit volume. Gases typically have much lower densities than liquids due to the greater distance between particles in a gas, which allows for more empty space. This fundamental difference in density is crucial for understanding the behavior of gases compared to liquids.

Compressibility of Gases

Compressibility refers to the ability of a substance to decrease in volume under pressure. Gases are highly compressible because their particles are far apart, allowing them to be pushed closer together. In contrast, liquids are much less compressible due to the closer arrangement of their particles, which limits their ability to be compressed.

Vapor Behavior and Miscibility

Miscibility describes the ability of two substances to mix in all proportions. The statement regarding liquid water and liquid carbon tetrachloride not mixing implies that their vapors also do not mix, which is not necessarily true. Vapor behavior can differ from liquid behavior, as gases can often mix regardless of the miscibility of their liquid forms.

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Related Practice

Textbook Question

A thin glass tube 1 m long is filled with Ar gas at 101.3 kPa, and the ends are stoppered with cotton plugs as shown below. HCl gas is introduced at one end of the tube, and simultaneously NH3 gas is introduced at the other end. When the two gases diffuse through the cotton plugs down the tube and meet, a white ring appears due to the formation of NH4Cl1s2. At which location—a, b, or c—do you expect the ring to form?

The graph below shows the change in pressure as the temperature increases for a 1-mol sample of a gas confined to a 1-L container. The four plots correspond to an ideal gas and three real gases: CO2, N2, and Cl2. (a) At room temperature, all three real gases have a pressure less than the ideal gas. Which van der Waals constant, a or b, accounts for the influence intermolecular forces have in lowering the pressure of a real gas?

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Textbook Question

The graph below shows the change in pressure as the temperature increases for a 1-mol sample of a gas confined to a 1-L container. The four plots correspond to an ideal gas and three real gases: CO2, N2, and Cl2. (b) Use the van der Waals constants in Table 10.3 to match the labels in the plot (A, B, and C) with the respective gases 1CO2, N2, and Cl22.

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Textbook Question

(b) Which units are appropriate for expressing atmospheric pressures, N, Pa, atm, kg/m²?

Suppose that a woman weighing 130 lb and wearing high-heeled shoes momentarily places all her weight on the heel of one foot. If the area of the heel is 0.50 in.2, calculate the pressure exerted on the underlying surface in a. pounds per square inch,

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