Hyperbaric chambers, which provide high pressures (up to 6 atm) of either air or pure oxygen, are used to treat a variety of conditions, ranging from decompression sickness in deep-sea divers to carbon monoxide poisoning. Look up the solubility of O₂, N₂, CO, and CO₂ in water at standard temperature and pressure (1 atm, 25 °C).Explain the trends in relative solubility for these gases. (Refer to Section 8.2 and Section 9.2)

Verified step by step guidance

1. Identify the solubility of each gas (O₂, N₂, CO, and CO₂) in water at standard temperature and pressure (1 atm, 25 °C).
2. Understand that solubility is influenced by factors such as molecular size, polarity, and the presence of chemical reactions with water.
3. Recognize that CO₂ is more soluble in water than O₂, N₂, and CO due to its ability to react with water to form carbonic acid, increasing its solubility.
4. Note that N₂ and O₂ are nonpolar and have similar solubility trends, but O₂ is slightly more soluble due to its smaller molecular size and higher polarizability.
5. Understand that CO has a solubility between that of O₂ and CO₂, as it is slightly polar and can form weak interactions with water.

Key Concepts

Gas Solubility

Gas solubility refers to the ability of a gas to dissolve in a liquid, which is influenced by factors such as temperature, pressure, and the nature of the gas and solvent. Generally, higher pressures increase gas solubility in liquids, as described by Henry's Law, which states that the amount of gas dissolved in a liquid is proportional to the pressure of the gas above the liquid.

Henry's Law

Henry's Law states that at a constant temperature, the amount of a gas that dissolves in a liquid is directly proportional to the partial pressure of that gas in equilibrium with the liquid. This principle helps explain why gases like oxygen and carbon dioxide have different solubilities in water, as their solubility coefficients vary, affecting how much of each gas can be dissolved under specific conditions.

Molecular Properties of Gases

The solubility of gases in water is also influenced by their molecular properties, such as polarity and molecular weight. For instance, polar gases tend to be more soluble in water than nonpolar gases due to interactions with water molecules. Additionally, lighter gases like helium are generally less soluble than heavier gases like carbon dioxide, which can form weak interactions with water, enhancing its solubility.