Question

How many grams of carbon dioxide gas is dissolved in a 1 L bottle of carbonated water if the manufacturer uses a pressure of 2.4 atm in the bottling process at 25${}^o$C?
Given: $K_H$ of $C{O}_2$ in water $=$ 29.76 atm/(mol/L) at 25${}^o$C

• A. $3.88$ g
• B. $4.90$ g
• C. $5.33$ g
• D. $3.52$ g

Answer 1

The correct option is D $3.52$ g

According to Henry's law, $P=K_{H}S$
$S$ is the solubility in moles per litre
$K_H$ is the henry's law constant
$P$ is the pressure in atm.
Substitute values in the above expression.
$2.4=29.76\times S$
$S=0.0806M$
Thus 0.0806 moles are present in 1 L of solution. This corresponds to $0.086\times 44=3.52g$