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Henry’s Law

Henry’s Law describes the relationship of the solubility of a gas in a liquid and the partial pressure of that gas when it is in equilibrium with the liquid. For an ideal gas, concentration and partial pressure are directly proportional if the temperature remains constant. Thus, this explains why more gas is dissolved in the liquid if its partial pressure is higher. Henry’s Law is commonly written as: P = k*C where, p is the partial pressure of the solute in the gas above the solution C is the concentration of the solute k is a constant CO2 can dissolve in water to form carbonated water. So for example, if the partial pressure of CO2 doubles, the amount of CO2 which dissolves in water will also double. Conversely, if the partial pressure of CO2 halves, then the amount which dissolves in water also halves. Thus, understanding Henry’s Law is crucial for understanding the solubility of gases in a variety of liquids. It can even be applied to everyday examples such as carbonated soft drinks, where CO2 is purposely trapped within a can/bottle to create a high partial pressure, causing more CO2 to dissolve. Opening the soft drink can/bottle will relieve the high partial pressure of CO2, leading to the amount of CO2 dissolved to decrease, and eventually rendering the soft drink flat.

Applying Henry's Law

Please help with the following problems: We are asked to estimate the evaporation from a static body of water such as a lake or pond. The dimension of the pond is 76.22m x 60.98m x 1.07m and contains ~ 4921 cubic meters of water. The mean atmospheric air temp above the pond is 10 degrees C with a relative humidity of 6

Solubility of gas in liquid.

Illustrate the relationship between a pressure of a gas above a liquid and the solubility of the gas in the liquid. Determine the concentration of CO2 in a carbonated beverage bottled under 4.0 atm of CO2. (a) If the mole fraction of CO2 in the air is 0.00355, how many times more concentrated is the CO2 in the unopened bottle