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At a constant temperature, the amount of a given gas dissolved in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid. THIS IS HOW WE MAKE SODA.
P=KC P=pressure of the gas (atm) K=Henry's Law Constant (atm/M) C=Concentration of the Gas (M) Examples-The Henry's law constant for He gas in water at 30°C is 2.70 x 103 atm/M. The constant for N2 at the same temperature is 1.67 x 103 atm/M. If the two gases are each present at 1.43 atm pressure, calculate the solubility, in M, of each gas. P=KC or P/K=C He
***Watch the units some chemist use the equation S=KP (solubility= Henrys constant x pressure) Henrys constant will have the units of M/atm for this equation Example-The Henry's Law constant for the solubility of nitrogen in water is 6.40x10^-4 M/atm at 25.0 Celsius. At .750 atm how many grams of N2 can be dissolved in .250 L of water at 25.0 degrees Celsius Answer-S = (6.40 x 10^-4 M/atm)*(0.750 atm) = 4.8 x 10^-4 M
Decompression Sickness
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