At 740 torr and \(20.0^{\circ} \mathrm{C}\), nitrogen has a solubility in water of \(0.018 \mathrm{~g} \mathrm{~L}^{-1}\). At 620 torr and \(20.0{ }^{\circ} \mathrm{C}\), its solubility is \(0.015 \mathrm{~g} \mathrm{~L}^{-1}\). Show that nitrogen obeys Henry's law.

Understanding how gases dissolve in liquids is essential for fully grasping many phenomena in chemistry, including the behavior of carbonated drinks, preserving foods, and even our own respiration. When a gas comes in contact with a liquid, it can enter and become dissolved within the liquid to form a solution. The solubility of a gas in a liquid is influenced by temperature, pressure, and the nature of the gas and the solvent. As a general rule, the solubility of a gas increases with pressure and decreases with temperature.

The behavior of gases dissolving in liquids can be elegantly described by Henry's Law. This principle allows us to predict and quantify the solubility of a gas within a liquid under various conditions. To illustrate, nitrogen's solubility in water changes when the pressure above the water is altered, as seen in the exercise. By comparing solubility at two different pressures, we directly apply the concept of gas solubility and Henry's Law.

The gas-liquid equilibrium is an essential concept to understand when discussing the solubility of gases in liquids. It refers to the state where the rate at which gas molecules enter the liquid is equal to the rate at which they escape back into the gas phase. This dynamic equilibrium is what Henry's Law describes. At this point, the concentration of the gas in the liquid remains constant as long as the temperature and the gas's partial pressure do not change.

When discussing gas solubility, knowing that equilibrium implies a steady state helps us to comprehend why and how conditions such as temperature and pressure influence a gas's solubility in a liquid. In the exercise provided, nitrogen's solubility in water at two different pressures, while at the same temperature, reflected the gas-liquid equilibrium under varying conditions, demonstrating that the system obeys Henry's Law.

Partial pressure is a term that describes the pressure a single gas contributes to a mixture of gases and plays a vital role in determining gas solubility according to Henry's Law. In a mixture, each gas exerts pressure as if it alone occupied the entire volume, and the total pressure is the sum of the individual partial pressures. This concept directly affects the amount of the gas that will dissolve when in contact with a liquid.

To understand how partial pressure influences gas solubility, let's refer back to our exercise. When the partial pressure of nitrogen is higher at 740 torr, more nitrogen dissolves in the water compared to when the pressure is lower at 620 torr. Adjusting the partial pressure essentially allows control over how much gas can be dissolved in the liquid, which is crucial for industrial applications such as beverage carbonation and manufacturing processes requiring precise gas concentrations.