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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. © BrainMass Inc. brainmass.com November 16, 2018, 9:21 am ad1c9bdddf

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

Henry's Law

What is the maximum number of grams of CO2 gas that can dissolve in 1.00 liter of water at 25 degrees Celsius if the partial pressure of the CO2 gas is 57.0 mm Hg? The Henry's Law constant for CO2 is 4.48 x 10-5 M/mm Hg.

Henry's Constants and Partial Pressure

Consider the following aqueous route to oxidize SO2: SO2(aq) + H2O2(aq) -> H2SO4(aq) k = 1.1 X 10^3 L/mols a. The partial pressure and Henry's law constants for SO2 and H2O2 are 2.1 ppm (KH = 1.2 mol L-1atm-1) and 4.8 ppb (KH = 1.0E5 mol L-1atm-1), respectively. Calculate the reaction rate of this process. b. Calculate th

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

Henry's law and molarity

What is the maximum # of Grams of CO2 gas that can dissolve in 1.00 liter of water at 25 degrees C if the partial pressure of the CO2 gas is 57.00 mmHg? The Henry's Law constant for CO2 is .000048 M/mmHg I was given the formula S=KP Using the factor-label method and expressing the answer to the correct number of signific