Question

How many grams of $C{O}_2$ gas is dissolved in a $1$ lt bottle of carbonated water if the manufacturer uses a pressure of $2.4$ atmosphere in the bottling process at ${25}^o$C? Given $K_H$ of $C{O}_2$ water $=29.76$ atm/mole/l at ${25}^o$C.

• A. $3.52$
• B. $4.2$
• C. $3.1$
• D. $2.5$

Answer 1

The correct option is A $3.52$

According to Hennry's Law,

$p=C{K}_h$

$p=2.4atm$

$K_h=29.76\frac{atm}{mol/L}$

$C=\frac{p}{K_h}=\frac{2.4}{29.76}=0.08\frac{mol}{L}$

$0.08mol$ of $C{O}_2$ are present in $1L$ of solution.

Grams of $C{O}_2=\left(moles\right)\left(molarmass\right)=\left(0.08\right)\left(44\right)=3.52$