Question

The solubility of CO2 in a salt water lake at 298 K and 750 torr pressure was found to be 1.0 x 10-5 moles CO2/liter of aqueous solution. The Henry’s Law constant in this case is 3.0 x 10-2 mol/L.atm. Please find the partial pressure of CO2 (g) (PCO2, in atm) in the air above the lake (2) Please use your answer to determine the percentage of CO2 in the atmosphere (2) Given the percentage of CO2 in the atmosphere is constant at sea level and below, please calculate the solubility (moles/liter of aqueous solution) of CO2 in the Dead Sea at 298 K and a pressure of 800 torr

Answer 1

the law:

M = H*Pi

H = constant of henry

M = molarity of gas in liquid

Pi = partial pressure of i

then

M of CO2 = 10^-5 M

P = 750 torr (atm) = 0.987 atm

H = 3*10^-2

fubd P-CO2

M = H*Pi

Pi = M/Hi = (10^-5)/(3*10^-2) = 0.000333 atm

2

find CO2 in atm

since atm is about 0.987 atm

then

x co2 = P of CO2/ total P= 0.000333/0.987 = 0.00033 (mol fraction)

0.00033 *100% = 0.033% approx is CO2 in atm

3

for

P = 800 torr = 800/760 = 1.052 atm

M = H*Pi

Pi = 1.052 *0.00033 = 0.0003471 atm of CO2

M = (3*10^-2)(0.0003471 ) = 0.00001041 M or mol of CO2 per liter of solution