Q1. The Henry’s law constant for oxygen dissolved in water is 4.34 × 104 atm at 25°C. If the partial pressure of oxygen in air is 0.2 atm under atmospheric conditions, calculate the concentration (in moles per liter) of dissolved oxygen in water in equilibrium with air at 25°C,
A. 4.6 × 10–6 mol L–1
B. 4.34 × 10–4 mol L–1
C. 2.55 × 10–4 mol L–1
D. 2.05 × 10–6 mol L–1
Ans. Correct option is C
Q2. Which one of the following statements regarding Henry’s law is not correct?
A. The value of KH increases with increase of temperature and KH is function of the nature of the gas
B. Different gases have different KH (Henry’s law constant) values at the same temperature
C. The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution.
D. Higher the value of KH at a given pressure, higher is the solubility of the gas in the liquids.
Ans. Correct option is D