Related InterviewSolutions

• Explain :Dynamic nature of chemical equilibrium with suitable example.
• The equilibrium constant value for the reaction:2H2(g) + O2(g) ⇌ 2H2O(g) is 2.4 × 1047 at 500 K. What is the value of equilibrium constant for the reaction:2H2O(g) ⇌ 2H2(g) + O2(g) ?(A) 0.41 × 10-46(B) 0.41 × 1047 (C) 0.41 × 10-48(D) 0.41 × 10-47 
• Relate the terms reversible reactions and dynamic equilibrium.
• State and explain Le Chatelier’s principle with reference to :a. Reversible reaction b. Rate of reaction
• How does the change of pressure affect the value of equilibrium constant?
• Write suitable conditions of concentration, temperature and pressure used during manufacture of ammonia by Haber process.
• Differentiate irreversible and reversible reaction.
• What is a closed system?
• Identify the CORRECT statement. (A) Catalyst lowers activation energy for the forward and reverse reactions by exactly the same amount. (B) The value of equilibrium constant decreases in presence of a catalyst. (C) Catalyst affect the position of the equilibrium. (D) Catalyst changes the equilibrium composition of a reaction mixture.
• The following reaction occurs in the blast furnace where iron ore is reduced to iron metal:3Fe2O3(s)  + 3CO(g) ⇌ 2Fe(l) + 3CO2(g)Using the Le Chatelier’s principle, predict which one of the following will NOT disturb the equilibrium?(A) Removal of CO (B) Removal of CO2 (C) Addition of CO2 (D) Addition of Fe2 O3