Why does increasing pressure increase gas solubility and does the solubility of a gas increase with increasing temperature and pressure?

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Ekrem Alagoz

Henry's law describes the relationship between the partial pressure of a gas above a liquid and the concentration of that gas dissolved in the liquid. It states that the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid, given a constant temperature.

Mathematically, Henry's law can be expressed as:

C=k⋅P

Where:C is the concentration of the gas in the liquid. k is Henry's law constant, which is specific to the gas and the solvent. P is the partial pressure of the gas above the liquid.

According to Henry's law, as you increase the pressure of a gas above a liquid, more gas molecules will dissolve into the liquid phase until equilibrium is reached. This is why, for example, carbon dioxide dissolves more readily in a soda at higher pressures, as in a sealed soda bottle. When you open the bottle, the pressure decreases, and carbon dioxide is released as bubbles.

The Effect of Temperature:In contrast to pressure, the solubility of most gases decreases with increasing temperature. This is because as temperature rises, the kinetic energy of gas molecules also increases, making them move more rapidly. Faster-moving gas molecules are less likely to be captured and held by the liquid, leading to lower solubility.The relationship between solubility and temperature is often described by the Clausius-Clapeyron equation, which shows that the solubility of gases generally decreases as temperature increases.

Rk Naresh

Dr Ekrem Alagoz thank you for your contribution to the discussion

The solubility of a gas in liquid increases with an increase in pressure at a given temperature. Conversely, the solubility of a gas decreases with a decrease in pressure and an increase in temperature decreases the solubility of a gas in a liquid. Increasing the pressure of the gas increases the number of molecules of gas per unit volume, which increases the rate at which gas molecules collide with the surface of the liquid and dissolve. It is known to you that Henry's law states that “at constant temperature and external pressure, the solubility of a gas in a liquid is directly proportional to the pressure at which it is dissolved. The solubility of the gas in a liquid solution decreases with increase in temperature. This is because, with an increase in temperature, the kinetic energy of the gas molecule increases, thus it becomes difficult for liquid molecules to hold them. As the pressure of the gas above water increases, the solubility also increases. The solubility of a gas in a liquid is directly proportional to the pressure of that gas above the surface of the solution. Increased temperature causes an increase in kinetic energy. The higher kinetic energy causes more motion in the gas molecules which break intermolecular bonds and escape from solution. Solubility of gases in water decreases with increase in temperature. For many solids dissolved in liquid water, the solubility increases with temperature. The increase in kinetic energy that comes with higher temperatures allows the solvent molecules to more effectively break apart the solute molecules that are held together by intermolecular attractions. this is the reason.