Equilibrium concepts chemical equilibrium Kc Kp and Le Chatelier's principle - One Line Questions

1. For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), the expression for Kp is: — (P_NH3)^2 / (P_N2 * (P_H2)^3)
2. For the reaction A(s) + B(g) ⇌ C(g), Kc expression is: — [C] / [B]
3. If Kc = 10 for a reaction A + B ⇌ C + D, and initially [A] = [B] = 1 M, then at equilibrium: — [C] = [D] < [A] = [B]
4. The equilibrium constant expression for the reaction 2A(g) + B(l) ⇌ 3C(g) is: — [C]^3 / [A]^2
5. For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), the expression for Kc is: — [NH3]^2 / ([N2] * [H2]^3)
6. The equilibrium constant Kc for the reaction 2SO3(g) ⇌ 2SO2(g) + O2(g) is 0.04. What is the equilibrium constant for the reaction SO2(g) + 1/2 O2(g) ⇌ SO3(g)? — 1/√0.04
7. For the reaction A(g) ⇌ B(g), if Kc = 0.5 and initial concentration of A is 1 M, what is the equilibrium concentration of B? — 0.333 M
8. For the reaction CO(g) + 1/2 O2(g) ⇌ CO2(g), what is Δn? — 1/2
9. For the reaction A(g) + B(g) ⇌ C(g) + D(g), if the initial concentrations of A and B are equal, and Kc = 4, what is the equilibrium concentration of C if initial concentrations of C and D are zero? — 2/3 M
10. What is the unit of Kp for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g)? — atm^-2
11. According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in volume, the equilibrium will shift to counteract the change in: — Pressure
12. The value of the equilibrium constant is affected by: — Temperature
13. The equilibrium constant (Kc) for a reaction is defined in terms of: — Molar concentrations of products raised to stoichiometric coefficients divided by molar concentrations of reactants raised to stoichiometric coefficients
14. For the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g), if the partial pressure of PCl5 is increased by a factor of 2, how will Kp be affected? — Unchanged
15. Which statement is incorrect regarding equilibrium? — At equilibrium, the rates of forward and backward reactions are zero.
16. Which of the following conditions must be met for a system to be at equilibrium? — Forward reaction rate equals backward reaction rate
17. In the Haber process for ammonia synthesis, N2(g) + 3H2(g) ⇌ 2NH3(g) + heat, which condition favors high yield of ammonia? — Low temperature, high pressure
18. What is the effect of increasing temperature on the equilibrium constant of an exothermic reaction? — Decreases
19. What is the effect of increasing temperature on the equilibrium constant of an endothermic reaction? — Increases
20. Le Chatelier's principle states that if a change of condition is applied to a system in equilibrium, the system will shift in a direction that: — Relieves the stress
21. The equilibrium constant for the reaction 2HI(g) ⇌ H2(g) + I2(g) is K. The equilibrium constant for the reaction HI(g) ⇌ 1/2 H2(g) + 1/2 I2(g) will be: — √K
22. The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is Kc. If the reaction is reversed and the reactants and products are swapped, the new equilibrium constant will be: — 1/Kc
23. What is the relationship between Kp and Kc for a gaseous reaction? — Kp = Kc(RT)^Δn
24. For a reaction where Δn = 0, what is the relationship between Kp and Kc? — Kp = Kc
25. What is the unit of Kc for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g)? — (mol/L)^-2
26. The equilibrium constant (Kp) is defined in terms of: — Partial pressures of gases
27. If the pressure of a gaseous equilibrium system is increased, the equilibrium will shift towards the side with: — Fewer moles of gas
28. Le Chatelier's principle is applicable to: — Both chemical and physical equilibria
29. If Kc for a reaction is 10^-5, it means that at equilibrium: — Reactants are highly favored
30. If the value of Kc is very large (Kc >> 1), it indicates that at equilibrium: — Products are favored
31. If the value of Kc is very small (Kc << 1), it indicates that at equilibrium: — Reactants are favored
32. Adding an inert gas to a system at equilibrium at constant volume will: — Not shift the equilibrium
33. Adding an inert gas to a system at equilibrium at constant pressure will: — Shift the equilibrium towards the side with more moles of gas
34. Consider the equilibrium 2NO(g) + O2(g) ⇌ 2NO2(g). If the volume of the container is doubled, what will be the effect on the equilibrium? — Shift towards reactants
35. The addition of a catalyst to a system at equilibrium: — Does not affect the equilibrium position but increases the rate of both forward and backward reactions
36. For the reaction H2(g) + I2(g) ⇌ 2HI(g), Δn = 0. If pressure is increased, the equilibrium: — Does not shift
37. In the expression Kp = Kc(RT)^Δn, Δn represents: — Sum of moles of products - Sum of moles of reactants
38. Which factor does NOT affect the position of equilibrium? — Catalyst
39. The equilibrium constant Kc is independent of: — Concentration of reactants
40. In a reversible reaction, the equilibrium is reached when: — The rate of the forward reaction equals the rate of the backward reaction.
41. Which of the following statements is true regarding a system at dynamic equilibrium? — The rate of the forward reaction is equal to the rate of the backward reaction.
42. For a reversible reaction, the rate of the forward reaction is equal to the rate of the backward reaction at: — The point of equilibrium
43. For the dissociation of PCl5(g) ⇌ PCl3(g) + Cl2(g), if the volume is decreased, the equilibrium will shift: — Towards products
44. Consider the reaction A(g) + B(g) ⇌ 2C(g). If the concentration of A is doubled, the equilibrium will shift: — Towards products
45. Consider the equilibrium CaCO3(s) ⇌ CaO(s) + CO2(g). If CO2 is removed from the system, the equilibrium will shift: — Towards products
46. According to Le Chatelier's principle, increasing the concentration of a reactant in a system at equilibrium will cause the equilibrium to shift: — Towards the products
47. For an exothermic reaction, increasing the temperature will cause the equilibrium to shift: — Towards the reactants
48. For an endothermic reaction, decreasing the temperature will cause the equilibrium to shift: — Towards the reactants
49. For the synthesis of methanol: CO(g) + 2H2(g) ⇌ CH3OH(g) (exothermic). To maximize the yield of methanol, one should: — Use low temperature and high pressure
50. If Kc = Kp, what can be concluded about the reaction? — Δn = 0
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