Chemistry

7.5. Find out the value of K_c for each of the following equilibria from the value of K_p:
(i) 2NOCl (g) ?? 2NO (g) + Cl₂ (g); Kp= 1.8 × 10^–2 at 500 K

(ii) CaCO₃ (s) ? CaO (s) + CO₂(g); Kp= 167 at 1073 K       

7.3. At a certain temperature and total pressure of 10⁵Pa, iodine vapour contains 40% by volume of I atoms

I₂ (g) ? 2I (g)

Calculate K_p for the equilibrium. 

5.4. At 0°C, the density of a gaseous oxide at 2 bar is same as that of dinitrogen at 5 bar. What is the molecular mass of the oxide?

5.3. Using the equation of state PV= nRT, show that at a given temperature, density of a gas is proportional to the gas pressure P.

5.1. What will be the minimum pressure required to compress 500 dm³ of air at 1 bar to 200 dm³ at 30°C?

7.2. What is K_c for the following equilibrium when the equilibrium concentration of each substance is: [SO₂] = 0.60M, [O₂] = 0.82M and [SO₃] = 1.90 M?

2SO₂(g) + O₂(g) ? 2SO₃(g)  

7.1. A liquid is in equilibrium with its vapour in a sealed container at a fixed temperature. The volume of the container is suddenly increased.

(a) What is the initial effect of the change on the vapour pressure?

(b) How do the rates of evaporation and condensation change initially?

(c) What happens when equilibrium is restored finally and what will be the final vapour pressure?

7.1. A liquid is in equilibrium with its vapour in a sealed container at a fixed temperature. The volume of the container is suddenly increased.

(a) What is the initial effect of the change on the vapour pressure?

(b) How do the rates of evaporation and condensation change initially?

(c) What happens when equilibrium is restored finally and what will be the final vapour pressure?

5.5. Pressure of l g of an ideal gas A at 27°C is found to be 2 bar. When 2 g of another ideal gas B is introduced in the same flask at same temperature, the pressure becomes 3 bar. Find the relationship between their molecular masses.