At 298 K,Henry's law constant for CO_2 in wa | vedclass

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(D) According to Henry's law,$P = K_H 	imes \chi$,where $P$ is the partial pressure of the gas,$K_H$ is Henry's law constant,and $\chi$ is the mole f

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$5.55 	imes 10^{-2}$

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(D) According to Henry's law,$P = K_H 	imes \chi$,where $P$ is the partial pressure of the gas,$K_H$ is Henry's law constant,and $\chi$ is the mole fraction of the gas in the solution.Given: $P = 1.67 	imes 10^2 \ kPa = 1.67 	imes 10^5 \ Pa$,$K_H = 1.67 	imes 10^8 \ Pa$.Calculating mole fraction $\chi = P / K_H = (1.67 	imes 10^5) / (1.67 	imes 10^8) = 10^{-3}$.Since the solution is dilute,the mole fraction $\chi \approx n_{CO_2} / n_{H_2O}$.For $1000 \ mL$ of water,mass $= 1000 \ g$,so $n_{H_2O} = 1000 / 18 = 55.55 \ mol$.Thus,$n_{CO_2} = \chi 	imes n_{H_2O} = 10^{-3} 	imes 55.55 = 5.555 	imes 10^{-2} \ mol$.Since the volume is $1 \ L$,the concentration is $5.55 	imes 10^{-2} \ mol \ L^{-1}$.

At $298 \ K$,Henry's law constant for $CO_2$ in water is $1.67 \times 10^8 \ Pa$. At $298 \ K$,the quantity of $CO_2$ in $1000 \ mL$ of soda water when packed at $1.67 \times 10^2 \ kPa$ $CO_2$ pressure in $mol \ L^{-1}$ is: (water density $= 1.0 \ g \ cm^{-3}$)

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