In an experiment the equilibrium constant for the reaction A+B\leftrig...
Equilibrium Constant and Reaction Stoichiometry
The equilibrium constant (K) is a fundamental concept in chemical equilibrium that quantifies the extent of a chemical reaction at equilibrium. It is defined as the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their stoichiometric coefficients.
The Reaction:
A + B ⇌ C + D
Initial Concentrations:
In the first experiment, the initial concentrations of A and B are both 0.1 mol L−1. Let's assume that at equilibrium, the concentrations of A, B, C, and D are represented by [A], [B], [C], and [D] respectively.
Expression for Equilibrium Constant:
Based on the stoichiometry of the reaction, the expression for the equilibrium constant is given by:
K = ([C] * [D]) / ([A] * [B])
Experiment 1:
Initial concentrations:
[A] = 0.1 mol L−1
[B] = 0.1 mol L−1
Experiment 2:
Initial concentrations:
[A] = 2 mol L−1
[B] = 3 mol L−1
Determining the Equilibrium Constant:
To find the equilibrium constant for the second experiment, we need to determine the concentrations of A, B, C, and D at equilibrium.
Using the Concentration Ratios:
The equilibrium concentrations can be determined by considering the ratio of the initial concentrations. In experiment 2, the initial concentration ratio of A to B is 2:3, which means that for every 2 moles of A, there are 3 moles of B.
Assuming Equilibrium Concentrations:
Let's assume that at equilibrium, the concentrations of A, B, C, and D are:
[A] = 2x
[B] = 3x
[C] = y
[D] = y
Applying the Stoichiometry:
Based on the stoichiometry of the reaction, the concentration of C and D can be related to A and B. Since the stoichiometric coefficients of C and D are equal to 1, the concentrations are directly proportional to the reactants' concentrations.
[C] = [A]
[D] = [B]
Substituting into the Equilibrium Expression:
Substituting the equilibrium concentrations into the equilibrium expression, we get:
K = ([C] * [D]) / ([A] * [B])
K = (y * y) / (2x * 3x)
K = y^2 / (6x^2)
Equating Initial and Equilibrium Concentrations:
To determine the values of x and y, we can equate the initial and equilibrium concentrations of A and B.
For A:
[A]initial = [A]equilibrium
0.1 mol L−1 = 2x
For B:
[B]initial = [B]equilibrium
0.1 mol L−1 = 3x
Solving these equations, we find:
x = 0.05 mol L−1
Calculating the Equilibrium Constant:
Substituting the values of x and y
In an experiment the equilibrium constant for the reaction A+B\leftrig...
Equilibrium constant doesn't depend upon concentration it only depend upon temperature so the equilibrium constant remain same so the ans is K
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