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Chapter 13: Problem 4

Which two statements about gas mixtures are true? [Section 13.1] (a) Gases always mix with other gases because the gas particles are too far apart to feel significant intermolecular attractions or repulsions. (b) Just like water and oil don't mix in the liquid phase, two gases can be immiscible and not mix in the gas phase. (c) If you cool a gaseous mixture, you will liquefy all the gases at the same temperature. (d) Gases mix in all proportions in part because the entropy of the system increases upon doing so.

Short Answer

Expert verified
The correct two statements about gas mixtures are: (a) Gases always mix with other gases because the gas particles are too far apart to feel significant intermolecular attractions or repulsions. (d) Gases mix in all proportions in part because the entropy of the system increases upon doing so.

Step by step solution

01

Statement (a) Analysis

: Gases always mix with other gases because the gas particles are too far apart to feel significant intermolecular attractions or repulsions. This statement is true. Gases consist of particles that are widely spaced apart and mostly do not interact with each other. Thus, gas particles are unaffected by any significant forces of attraction or repulsion, easily mixing together.
02

Statement (b) Analysis

: Just like water and oil don't mix in the liquid phase, two gases can be immiscible and not mix in the gas phase. This statement is false. In the liquid phase, water and oil don't mix due to the differences in polarities. However, gas particles are far more spaced out and interact minimally with other particles, allowing them to easily mix with other gases.
03

Statement (c) Analysis

: If you cool a gaseous mixture, you will liquefy all the gases at the same temperature. This statement is false. Different gases will have different critical temperatures and boiling points, which means that they generally won't liquefy at the same temperature when cooled together.
04

Statement (d) Analysis

: Gases mix in all proportions, in part because the entropy of the system increases upon doing so. This statement is true. Mixing gases increases the randomness or disorder of the system, according to the second law of thermodynamics. This increase in entropy is a primary factor contributing to the spontaneous mixing of gases in all proportions. In conclusion, the correct two statements about gas mixtures are: (a) Gases always mix with other gases because the gas particles are too far apart to feel significant intermolecular attractions or repulsions. (d) Gases mix in all proportions in part because the entropy of the system increases upon doing so.

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Most popular questions from this chapter

Some soft drinks contain up to 85 ppm oxygen. (a) What is this concentration in mol/L? (b) What partial pressure of \(\mathrm{O}_{2}\) above water is needed to obtain \(85 \mathrm{ppm} \mathrm{O}_{2}\) in water at $10^{\circ} \mathrm{C} ?\( (The Henry's law constant for \)\mathrm{O}_{2}$ at this temperature is $\left.1.69 \times 10^{-5} \mathrm{~mol} / \mathrm{m}^{3}-\mathrm{Pa} .\right)$

Suppose you had a balloon made of some highly flexible semipermeable membrane. The balloon is filled completely with a \(0.2 \mathrm{M}\) solution of some solute and is submerged in a 0.1 \(M\) solution of the same solute: Initially, the volume of solution in the balloon is \(0.25 \mathrm{~L}\). Assuming the volume outside the semipermeable membrane is large, as the illustration shows, what would you expect for the solution volume inside the balloon once the system has come to equilibrium through osmosis? [Section 13.5]

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