Calculate the solubility of O2 in water at a partial pressure of O2 of 120 torr at 25^∘ C. The H

step 1 Let's calculate the gas concentration, which is the solubility of O2. C is equal to k times p. S

Calculate the solubility of O2 in water at a partial...

Calculate the solubility of $\mathrm{O}_{2}$ in water at a partial pressure of $\mathrm{O}_{2}$ of 120 torr at $25^{\circ} \mathrm{C}$. The Henry's law constant for $\mathrm{O}_{2}$ is $1.3 \times 10^{-3} \mathrm{mol} / \mathrm{L} \cdot \mathrm{atm}$ for Henry's law in the form $C=k P$ where $C$ is the gas concentration (mol/L).

Key Concepts

Unit Conversion

Unit conversion is critical in solving problems involving physical quantities, as the units must be consistent for accurate calculations. In gas solubility problems, converting pressure units—such as from torr to atmospheres—is necessary because the Henry’s law constant is often given in units per atmosphere.

Henry's Law

Henry's Law states that the concentration of a gas dissolved in a liquid is directly proportional to the partial pressure of that gas above the liquid. This relationship is fundamental for understanding how gases interact with liquids and is expressed mathematically as C = kP, where C is the concentration, k is the Henry’s law constant, and P is the partial pressure of the gas.

Partial Pressure

Partial pressure is a concept from gas laws that refers to the pressure contributed by an individual component in a mixture of gases. In the context of gas solubility, the partial pressure of a specific gas determines how much of that gas will dissolve in a liquid according to Henry's Law.

Gas Solubility

Gas solubility refers to the ability of a gas to dissolve in a liquid, which is governed by factors like temperature, pressure, and the nature of both the gas and the liquid. Understanding gas solubility is important in a variety of fields, including environmental science, chemical engineering, and biology.

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