Tasks and exercises

1. The equilibrium concentrations for the reaction between carbon monoxide and molecular chlorine to form COCl₂ (g) at 740C are [CO] = 0.012 M, [Cl₂] = 0.054 M, and [COCl₂] = 0.14 M. Calculate the equilibrium constants Kc and Kp.

2. Consider the following equilibrium at 295 K: NH₄HS (s) → NH₃ (g) + H₂S (g). The partial pressure of each gas is 0.265 atm. Calculate Kp and Kc for the reaction?

3. The rate of decomposition of a gas was 7.25 in some unit when 5% had reacted and it was 5.14 in the same unit when 20% had undergone decomposition. Calculate the order.

4. Calculate the equilibrium concentration for CF₄ if Kc = 2.0 and the equilibrium mixture contains 0.10M COF₂ and 0.050M CO₂. 2COF₂(g) ⇄ CO₂(g) + CF₄(g)

5. What is the numerical value of Kc for the reaction, N₂O₄ (g) ⇄ 2NO₂ (g), of the equilibrium mixture that contains 0.030 M N₂O₄ ⇄ and 0.21 M NO₂?

2. The specific reaction rates of a chemical reaction are 2.45 × 10^-5 sec^-1 at 273 K and 16.2 × 10^-4 sec^-1 at 303 K. Calculate the activation energy.

3. The initial rate of a first order reaction is 5.2 × 10^-6 mol.lit^-1.s^-1 at 298 K. When the initial concentration of reactant is 2.6 × 10^-3 mol.lit^-5, calculate the first order rate constant of the reaction at the same temperature.

4. Calculate the value of K for the reaction CaCO₃(s) + H⁺(aq) = Ca₂⁺(aq) + HCO₃^-(aq)

5. The equilibrium constant, Kc, for H₂(g) + I₂(g) ⇄ 2HI(g) is 54. If the equilibrium mixture contains 0.15 M I₂ and 0.030 M HI, what is the molar concentration of H₂?

6. The equilibrium constant, Kc, for the reaction, N₂O₄ (g) ⇄ 2NO₂ (g), is 4.6 × 10-3. If the equilibrium mixture contains 0.050 M NO₂, what is the molar concentration of N₂O₄?