Question

A company dissolves ' $X$ ' amount of $CO _{2}$ at $298 K$ in $1$ litre of water to prepare soda water $X =$ ______$\times 10^{-3} g .$ (nearest integer)
(Given: partial pressure of $CO _{2}$ at $298\, K =0.835$ bar.
Henry's law constant for $CO _{2}$ at $298 \, K =1.67\, kbar$.
Atomic mass of $H , C$ and $O$ is $1,12$ and $6\, g\, mol ^{-1}$, respectively)

Answer 1

From Henry law
$P = K _{ H } X _{ CO _{2}}$
$0.835=1.67 \times 10^{3} \times 1.67 \times 10^{3} \times \frac{ w _{ CO _{2}} / 44}{\frac{ w _{ CO _{2}}}{44}+\frac{1000}{18}} $
$ w _{ CO _{2}}=1.2228 \,g =1222.8 \times 10^{-3} g$
Or
$P = K _{ H } X _{ CO _{2}}$
$0.835=1.67 \times 10^{3} \times \frac{ n _{ CO _{2}}}{ n _{ CO _{2}}+ n _{ H _{2} O }}$
$0.835=1.67 \times 10^{3} \times \frac{ w _{ CO _{2}} / 44}{\frac{1000}{18}}$
$w _{ CO _{2}}=1.2222 \,g =1222.2 \times 10^{-3} g$