Henry\'s law states that the solubility of a gas, S_g, is directly proportional

Question

Henry's law states that the solubility of a gas, S_g, is directly proportional to its partial pressure, P_g: S_g = kP_g where k is the Henry's law constant for a specific gas at a specified temperature. Note that the units of the constant am determined by the units of the pressure and concentration used. Atmospheric pressure is 1 00 atm, but air is only composed of 21.0% (by moles) oxygen. Thus, the partial pressure of 1.00 atm. What is the millimolar concentration of dissolved oxygen for a lake or stream under the partial pressure of oxygen and a temperature of 12 degree C? Express the millimolar concentration numerically to two significant figures.

Explanation / Answer

Find milimolar concentration of O2

given

S = 7.8×104 for OXygen (please use your actual value, since this is pretty dependent on literature being used)

so..

C = H*P

where

C = cncentration in mol / L

H = henrys constat

P = partial pressure of O2

for P = 1 atm and x = 0.21 of O2 --< P-O2 = 0.21 atm

so

C = (7.8*10^-4)*0.21

c = 0.0001638 mol / L

1 mol = 1000 mmol

C = 0.0001638*10^3

C = 0.1638 mol/L

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