Can you please explain the gases in liquid equilibrium using the example of CO2 bubble in a soda bottle and the changes with pressure.
The solubility of a gas in a liquid depends on temperature, the partial pressure of the gas over the liquid, the nature of the solvent and the nature of the gas. The most common solvent is water. Carbonated beverages are an example of Henry's law in everyday life. The dissolved carbon dioxide stays in solution in a closed pop bottle or can where the partial pressure of carbon dioxide was set at a high value during bottling. When the can or bottle is opened the partial pressure of CO2 is much lower and the dissolved carbon dioxide will gradually escape from the pop. When the new low partial pressure equilibrium is established the soda will be "flat". This loss of dissolved carbon dioxide will happen faster for warm soda than for cold.
Gas solubility is always limited by the equilibrium between the gas and a saturated solution of the gas. The dissolved gas will always follow Henry's law.
The concentration of dissolved gas depends on the partial pressure of the gas. The partial pressure controls the number of gas molecule collisions with the surface of the solution. If the partial pressure is doubled the number of collisions with the surface will double. The increased number of collisions produce more dissolved gas.
The solubility of a gas in a liquid depends on temperature, the partial pressure of the gas over the liquid, the nature of the solvent and the nature of the gas. The most common solvent is water. Carbonated beverages are an example of Henry's law in everyday life. The dissolved carbon dioxide stays in solution in a closed pop bottle or can where the partial pressure of carbon dioxide was set at a high value during bottling. When the can or bottle is opened the partial pressure of CO2 is much lower and the dissolved carbon dioxide will gradually escape from the pop. When the new low partial pressure equilibrium is established the soda will be "flat". This loss of dissolved carbon dioxide will happen faster for warm soda than for cold.
Gas solubility is always limited by the equilibrium between the gas and a saturated solution of the gas. The dissolved gas will always follow Henry's law.
The concentration of dissolved gas depends on the partial pressure of the gas. The partial pressure controls the number of gas molecule collisions with the surface of the solution. If the partial pressure is doubled the number of collisions with the surface will double. The increased number of collisions produce more dissolved gas.
