Question #56767

3. The Henry’s law constant for CO2 in water at 25ºC is 3.4×10–2 mol/L·atm.

(a) Calculate the concentration of CO2 in a beer can with a partial pressure 3.0 atm over the beer at 25 ºC.

(b) Wascana Lake is located in city of Regina. Given that the partial pressure of CO2 is 3.9 × 10–4 atm, calculate the concentration of CO2 at 25 ºC in Wascana Lake.

(a) Calculate the concentration of CO2 in a beer can with a partial pressure 3.0 atm over the beer at 25 ºC.

(b) Wascana Lake is located in city of Regina. Given that the partial pressure of CO2 is 3.9 × 10–4 atm, calculate the concentration of CO2 at 25 ºC in Wascana Lake.

Expert's answer

C=k·P(gas)

where

C - the solubility of a gas at a fixed temperature in a particular solvent, mL gas/L;

K - Henry's law constant, mol/L·atm;

Pgas - the partial pressure of the gas, atm.

a) C = 3.0·3.4×10^{–2}=0.102 ml/L

b) C = 3.9·10^{–4}·3.4×10^{–2}=1.3·10^{-5} ml/L

where

C - the solubility of a gas at a fixed temperature in a particular solvent, mL gas/L;

K - Henry's law constant, mol/L·atm;

Pgas - the partial pressure of the gas, atm.

a) C = 3.0·3.4×10

b) C = 3.9·10

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