Question

Calculate the solubility of carbon dioxide in water at an atmospheric pressure of 0.400 atm (a typical value at high altitude).Atmospheric Gas Mole Fraction kH mol/(L*atm)N2 7.81 x 10-1 6.70 x 10-4O2 2.10 x 10-1 1.30 x 10-3Ar 9.34 x 10-3 1.40 x 10-3CO2 3.33 x 10-4 3.50 x 10-2CH4 2.00 x 10-6 1.40 x 10-3H2 5.00 x 10-7 7.80 x 10-4

Answer 1

Answer:

The molar solubility of carbon dioxide gas is $4.662\times 10^{-6} M$.

Explanation:

Henry's law states that the amount of gas dissolved or molar solubility of gas is directly proportional to the partial pressure of the liquid.

To calculate the molar solubility, we use the equation given by Henry's law, which is:

$C_{CO_2}=K_H\times p_{liquid}$

where,

$K_H$ = Henry's constant = $3.50\times 10^{-2}mol/L.atm$

$p_{CO_2}$ = partial pressure of carbonated drink

$p_{CO_2}=p\times \chi_{CO_2}$

where = p = Total pressure = 0.400 atm

$\chi_{CO_2}$ = mole fraction of $CO_2=3.33\times 10^{-4}$

$p_{CO_2}=0.400 atm\times 3.33\times 10^{-4} =0.0001332 atm$

Putting values in above equation, we get:

$C_{CO_2}=3.5\times 10^{-2}mol/L.atm\times 0.0001332 atm\\\\C_{CO_2}=4.662\times 10^{-6} M$

Hence, the molar solubility of carbon dioxide gas is $4.662\times 10^{-6} M$.