Calculate the solubility of a gas in water at $0.8 \ atm$ and $25^{\circ} C$. [Henry's law constant is $6.85 \times 10^{-4} \ mol \ dm^{-3} \ atm^{-1}$]
- A$5.48 \times 10^{-4} \ mol \ dm^{-3}$
- B$3.94 \times 10^{-4} \ mol \ dm^{-3}$
- C$6.858 \times 10^{-4} \ mol \ dm^{-3}$
- D$2.74 \times 10^{-4} \ mol \ dm^{-3}$
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At $293 \ K$,the Henry law constant in water for $N_2$ and $O_2$ are $76.48 \ kbar$ and $34.86 \ kbar$ respectively. What is the ratio of mole fractions of $N_2$ and $O_2$ in water? (Assume partial pressures of $N_2$ and $O_2$ are the same at $293 \ K$)
Which of the following graphs correctly represents the plots of $K_{H}$ for gases in water versus temperature?
$K_H$ is Henry's constant and has the unit
Choose the correct statement about Henry's constant $(K_H)$.
$I$. $K_H$ increases with increase in temperature generally.
$II$. $K_H$ decreases with increase in temperature generally.
$III$. $K_H$ is the characteristic constant of the gas-solvent system.
$I$. $K_H$ increases with increase in temperature generally.
$II$. $K_H$ decreases with increase in temperature generally.
$III$. $K_H$ is the characteristic constant of the gas-solvent system.
Easy
View SolutionThe statement "The mass of a gas dissolved in a given mass of a solvent at any temperature is proportional to the pressure of the gas above the solvent" is
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