Henry's Law

Calculate the proportion of ${\mathrm{O}}_2$ and ${\mathrm{N}}_2$ dissolved in water at $298 \mathrm{K}$. When air containing $20\% {\mathrm{O}}_2$ and $80\%{ \mathrm{N}}_2$ by volume is in equilibrium with water at $1 \mathrm{atm}$ pressure. Henry's law constants for two gases are ${\mathrm{K}}_{\mathrm{H}}\left({\mathrm{O}}_2\right)=4.6\times {10}^4 \mathrm{atm}$  and ${\mathrm{K}}_{\mathrm{H}}\left({\mathrm{N}}_2\right)=8.5\times {10}^4 \mathrm{atm}$.

State and explain Henry’s law.

The ${\mathrm{K}}_{\mathrm{H}}$ for the solution of oxygen dissolved in water is $4\times {10}^4 \mathrm{atm}$ at a given temperature. If the partial pressure of oxygen in air is $0.4 \mathrm{atm}$, the mole fraction of oxygen in solution is

The Henry's law constants for two gases $\mathrm{A}$ and $\mathrm{B}$ are $\mathrm{x}$ and $\mathrm{y}$ respectively. The ratio of mole fractions of $\mathrm{A}$ to $\mathrm{B}$ is $0.2$. The ratio of mole fraction of $\mathrm{B}$ and $\mathrm{A}$ dissolved in water will be

Which one of the following gases has the lowest value of Henry's law constant?

The Henry's law constant for the solubility of Nitrogen gas in water at $350 \mathrm{K}$ is $8 \times {10}^4 \mathrm{atm}$. The mole fraction of nitrogen in air is $0.5$. The number of moles of Nitrogen from air dissolved in $10$ moles of water at $350 \mathrm{K}$ and $4$atm pressure is

The partial pressure of nitrogen in the air is $0.76 \mathrm{atm}$ and its Henry's law constant is $7.6 \times {10}^4 \mathrm{atm}$ at $300 \mathrm{K}$. What is the mole fraction of nitrogen gas in the solution obtained when the air is bubbled through water at $300 \mathrm{K}$?