The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas. This statement is known as ...

If $N_2$ gas is bubbled through water at $293 \ K$,how many moles of $N_2$ gas would dissolve in $1 \ litre$ of water? Assume that $N_2$ exerts a partial pressure of $0.987 \ bar$. [Given $K_{H}$ for $N_2$ at $293 \ K$ is $76.48 \ kbar$]

At $298 \ K$,how many millimoles of $CO_2$ gas will dissolve in $900 \ mL$ of water when $CO_2$ gas is passed through it? The $K_H$ value is $6.02 \times 10^{-4} \ bar$ and the partial pressure of $CO_2$ gas is $2 \times 10^{-8} \ bar$.

Assertion $(A)$: For an endothermic dissolution process,an increase in temperature increases the solubility in a nearly saturated solution.
Reason $(R)$: In a saturated solution,dynamic equilibrium exists between the dissolved solute and the undissolved solute.

Which one is an example of a solid solution?

Why do gases always tend to be less soluble in liquids as the temperature is raised?