Multiple Choice
For the reaction A (g) ⇌ 2 B (g), K = 14.7 at 298 K, what is the value of the reaction quotient Q at 298 K when ΔG = 19.6 kJ/mol?
19. Chemical Thermodynamics
Gibbs Free Energy And Equilibrium
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What is the relationship between the equilibrium constant (Kₚ), the reaction quotient (Qₚ), and the standard equilibrium constant (K₀) for a reaction involving gases?
A
Kₚ > Qₚ when the reaction is at equilibrium.
B
K₀ > Kₚ when the reaction is at equilibrium.
C
Kₚ = Qₚ when the reaction is at equilibrium.
D
K₀ = Qₚ when the reaction is at equilibrium.
Verified step by step guidance1
Understand the concept of equilibrium constant (Kₚ): The equilibrium constant for a reaction involving gases, denoted as Kₚ, is a measure of the ratio of the concentrations of products to reactants at equilibrium, expressed in terms of partial pressures.
Understand the concept of reaction quotient (Qₚ): The reaction quotient, Qₚ, is similar to Kₚ but is calculated at any point in time, not necessarily at equilibrium. It helps predict the direction in which a reaction will proceed to reach equilibrium.
Understand the concept of standard equilibrium constant (K₀): The standard equilibrium constant, K₀, is typically used to describe the equilibrium position under standard conditions, such as 1 atm pressure and a specified temperature.
Analyze the relationship between Kₚ and Qₚ: At equilibrium, the reaction quotient Qₚ equals the equilibrium constant Kₚ, i.e., Kₚ = Qₚ. If Qₚ < Kₚ, the reaction will proceed forward to reach equilibrium. If Qₚ > Kₚ, the reaction will proceed in reverse.
Clarify the statement about K₀ and Kₚ: The statement 'K₀ > Kₚ when the reaction is at equilibrium' is incorrect. K₀ is not directly compared to Kₚ in this context. The correct relationship at equilibrium is Kₚ = Qₚ.
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