List of top Chemistry Questions on Partial pressure asked in KEAM

The reaction:

\[ \text{H}_2\text{O}(g) + \text{Cl}_2\text{O}(g) \rightleftharpoons 2 \text{HOCl}(g) \]

is allowed to attain equilibrium at 400K. At equilibrium, the partial pressures are given as:

  • \( P_{\text{H}_2\text{O}} = 300 \) mm Hg
  • \( P_{\text{Cl}_2\text{O}} = 20 \) mm Hg
  • \( P_{\text{HOCl}} = 60 \) mm Hg

The value of \( K_p \) for the reaction at 400K is:

\[ K_p = \frac{P_{\text{HOCl}}^2}{P_{\text{H}_2\text{O}} \cdot P_{\text{Cl}_2\text{O}}} \]

A cycle tube will burst if the volume of air inside exceeds 1L at the room temperature. If at I bar pressure the air occupies 500 mL, then up to what pressure can the tube be expanded at the same temperature?
The partial pressure of nitrogen in air is $0.76\, atm$. and its Henry?s law constant is $7.6 \times 10^4$ atm at 300 K. What is the mole fraction of $N_2$ in the solution obtained when air is bubbled through water at 300 K?
The partial pressure of oxygen in the alveolar air is: