If the pressure surrounding a glass of water is increased, what will happen to the amount of gas dissolved in the water?

When the pressure surrounding a glass of water is increased, the solubility of gases in the water increases. This phenomenon is explained by Henry's Law, which states that at a constant temperature, the amount of gas that can be dissolved in a liquid is directly proportional to the partial pressure of that gas above the liquid.

As pressure rises, more gas molecules are forced into the water, leading to an increase in the amount of gas dissolved. This is particularly relevant in situations such as deep-sea diving, where increasing pressure can enhance the solubility of oxygen and nitrogen in the blood of divers, which is critical for understanding the risks of decompression sickness.

In contrast, when gas is allowed to escape or the pressure is reduced, gas could come out of the solution, potentially forming bubbles. Therefore, increasing pressure directly encourages more gas to dissolve, which reflects the principle of gas solubility in liquids under changing pressures.