Question

The Henry's law constant for CO 2 ( g ) CO2(g) in water at 25 ∘ C 25 ∘C is 29.4 bar⋅M − 1 29.4 bar·M−1. Estimate the concentration of dissolved CO 2 ( g ) CO2(g) in a carbonated soft drink pressurized with 2.20 2.20 bar of CO 2 ( g ) CO2(g).

Answer 1

Answer:

The molar solubility of carbon dioxide gas is 0.07483 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:

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

where,

$K_H$ = Henry's constant = $29.4 bar M^{-1}$

$p_{CO_2}$ = partial pressure of carbonated drink = 2.20 bar

Putting values in above equation, we get:

$C_{CO_2}=\frac{ 2.20 bar}{29.4 bar M^{-1}}$

$C_{CO_2}=0.07483 M$

Hence, the molar solubility of carbon dioxide gas is 0.07483 M.