Calculating Equilibrium Constant for Reverse Reaction
Understanding Equilibrium Constants
Chemical reactions can proceed in both the forward and reverse directions until they reach a state of equilibrium. The equilibrium constant, Kc, quantifies the concentrations of the reactants and products at equilibrium for a particular reaction. It provides valuable information about the extent to which a reaction proceeds in either direction.
Reaction and Equilibrium Constant Calculation
Consider the reaction: 2 AB ⇌ A₂B₂
Given equilibrium constant (Kc) for this reaction: 1.3 × 10^-15
We need to find Kc for the reverse reaction: A₂B₂ ⇌ 2 AB
Final answer:
The equilibrium constant (Kc) for the reverse reaction A₂B₂ ⇌ 2 AB is 7.69 × 10^14.
Explanation:
To find the equilibrium constant (Kc) for the reverse reaction A₂B₂ ⇌ 2 AB, we can use the relationship between the equilibrium constants for the forward and reverse reactions. The equilibrium constant for the reverse reaction is the inverse of the equilibrium constant for the forward reaction. Therefore, the value of Kc for the reverse reaction is 1 divided by the value of Kc for the forward reaction.
In this case, since the equilibrium constant for the forward reaction (2 AB ⇌ A₂ B₂) is given as 1.3 × 10^-15, the equilibrium constant for the reverse reaction is 1 / 1.3 × 10^-15 = 7.69 × 10^14. Therefore, the correct answer is option d) 406.
For the reaction 2 AB ⇌ A₂ B₂, what is K_c at the same temperature for the reverse reaction A₂B₂ ⇌ 2 AB? The equilibrium constant (Kc) for the reverse reaction A₂B₂ ⇌ 2 AB is 7.69 × 10^14.