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Chapter 13: Problem 27

Discuss the factors that influence the solubility of a gas in a liquid. Explain why the solubility of a gas in a liquid usually decreases with increasing temperature.

Short Answer

Expert verified
Two factors affect the solubility of gases in liquids: temperature and external pressure. The solubility decreases with rising temperature because increased kinetic energy of the molecules amplifies their escape tendency from the liquid.

Step by step solution

01

Identifying factors affecting the solubility of gases in liquids

There are two main factors that affect the solubility of a gas in a liquid. Firstly, the temperature of the liquid: an increase in temperature decreases the solubility of a gas and vice versa. This is contrary to the effect of temperature on the solubility of solid substances. Secondly, the external pressure: applying pressure raises the solubility of a gas in a liquid. This is known as Henry's Law, which states that at a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the presssure of that gas in equilibrium with that liquid.
02

Why solubility of a gas in a liquid decreases with rising temperature

The solubility of gases in liquids diminishes as temperature increases because the kinetic energy of the molecules also increases. This amplifies the escape tendency of the gas particles from the liquid - the higher the temperature, the greater the kinetic energy. Therefore, more gas particles have enough energy to overcome the attractive forces holding them in the liquid, causing them to escape more easily. As a result, it becomes more difficult to dissolve additional gas in the liquid at higher temperatures.

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Most popular questions from this chapter

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The vapor pressure of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) at \(20^{\circ} \mathrm{C}\) is \(44 \mathrm{mmHg},\) and the vapor pressure of methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) at the same temperature is \(94 \mathrm{mmHg}\). A mixture of \(30.0 \mathrm{~g}\) of methanol and \(45.0 \mathrm{~g}\) of ethanol is prepared (and may be assumed to behave as an ideal solution). (a) Calculate the vapor pressure of methanol and ethanol above this solution at \(20^{\circ} \mathrm{C}\). (b) Calculate the mole fraction of methanol and ethanol in the vapor above this solution at \(20^{\circ} \mathrm{C}\).

A solution of \(2.50 \mathrm{~g}\) of a compound of empirical formula \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{P}\) in \(25.0 \mathrm{~g}\) of benzene is observed to freeze at \(4.3^{\circ} \mathrm{C}\). Calculate the molar mass of the solute and its molecular formula.

Consider two aqueous solutions, one of sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) and the other of nitric acid \(\left(\mathrm{HNO}_{3}\right)\) both of which freeze at \(-1.5^{\circ} \mathrm{C}\). What other properties do these solutions have in common?

Arrange these aqueous solutions in order of decreasing freezing point and explain your reasons: (a) \(0.50 \mathrm{~m}\) \(\mathrm{HCl},\) (b) \(0.50 \mathrm{~m}\) glucose, (c) \(0.50 \mathrm{~m}\) acetic acid.
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