At T (K) the molarity of CO_2 (in mol L^{-1 | vedclass

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(B) According to Henry's law,$p = K_H \cdot \chi$,where $\chi$ is the mole fraction of $CO_2$. Given $p = 3.4 \ bar$ and $K_H = 1.7 	imes 10^3 \ bar$

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$1.11 	imes 10^{-1}$

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(B) According to Henry's law,$p = K_H \cdot \chi$,where $\chi$ is the mole fraction of $CO_2$. Given $p = 3.4 \ bar$ and $K_H = 1.7 	imes 10^3 \ bar$. $\chi = \frac{p}{K_H} = \frac{3.4}{1.7 	imes 10^3} = 2 	imes 10^{-3}$. Since the solution is dilute,$\chi = \frac{n_{CO_2}}{n_{H_2O}}$. $n_{H_2O} = \frac{200 \ g}{18 \ g \ mol^{-1}} = 11.11 \ mol$. $n_{CO_2} = \chi 	imes n_{H_2O} = 2 	imes 10^{-3} 	imes 11.11 = 2.222 	imes 10^{-2} \ mol$. Molarity $= \frac{n_{CO_2}}{	ext{Volume in } L} = \frac{2.222 	imes 10^{-2} \ mol}{0.2 \ L} = 0.1111 \ mol \ L^{-1} = 1.11 	imes 10^{-1} \ mol \ L^{-1}$.

At $T \ (K)$ the molarity of $CO_2$ (in $mol \ L^{-1}$) in $200 \ mL$ of soda water packed under a pressure of $3.4 \ bar$ is ($K_H$ of $CO_2$ in water is $1.7 \times 10^3 \ bar$ at $T \ (K)$).

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