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In an experiment the equilibrium constant for the reaction A B - C D is K when the initial concentration of A and B each is 0.1 mol/l under the similar conditions in an another experiment if the initial concentration of A and B are taken 2 and 3 mol/l respectively then the value of equilibrium constant will be?
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In an experiment the equilibrium constant for the reaction A B - C ...
Explanation:


To determine the value of the equilibrium constant when the initial concentration of A and B are 2 and 3 mol/L respectively, we can use the concept of stoichiometry and the relationship between concentrations and the equilibrium constant.

The balanced equation for the given reaction is:

A + B ⟶ C + D

Step 1: Determining the Equilibrium Concentrations


In the first experiment, the initial concentration of A and B is 0.1 mol/L each. Let's assume that at equilibrium, the concentration of A and B both become x mol/L. Therefore, the concentrations of C and D will also be x mol/L.

In the second experiment, the initial concentration of A and B is 2 and 3 mol/L respectively. Let's assume that at equilibrium, the concentration of A becomes y mol/L and the concentration of B becomes z mol/L. Therefore, the concentrations of C and D will also be y and z mol/L respectively.

Step 2: Writing the Equilibrium Expression


The equilibrium expression for the given reaction is:

K = [C] * [D] / [A] * [B]

In both experiments, the equilibrium constant (K) remains the same.

Step 3: Applying the Law of Mass Action


Using the equilibrium concentrations determined in step 1, we can substitute these values into the equilibrium expression.

For the first experiment, where the equilibrium concentrations are x mol/L for A, B, C, and D:

K = [x] * [x] / [0.1] * [0.1]

For the second experiment, where the equilibrium concentrations are y mol/L for A and z mol/L for B:

K = [y] * [z] / [2] * [3]

Since the equilibrium constant (K) remains the same in both experiments, we can equate the two expressions:

[x] * [x] / [0.1] * [0.1] = [y] * [z] / [2] * [3]

Simplifying the equation, we get:

[x]^2 = [y] * [z] * 0.1 * 0.1 / 2 * 3

Step 4: Relationship Between Initial Concentrations and Equilibrium Concentrations


We know that the initial concentration of A and B in the first experiment is 0.1 mol/L each, and in the second experiment, it is 2 and 3 mol/L respectively. Therefore, we can relate the equilibrium concentrations (x, y, and z) to the initial concentrations using the concept of stoichiometry.

Since the molar ratio between A, B, C, and D is 1:1:1:1, the equilibrium concentration of A in the first experiment can be written as:

x = 0.1 - y - z

Similarly, the equilibrium concentration of A in the second experiment can be written as:

x = 2 - y - z

Step 5: Solving for the Equilibrium Constant


By substituting the expressions for x in both experiments into the equation obtained
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In an experiment the equilibrium constant for the reaction A B - C D is K when the initial concentration of A and B each is 0.1 mol/l under the similar conditions in an another experiment if the initial concentration of A and B are taken 2 and 3 mol/l respectively then the value of equilibrium constant will be?
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In an experiment the equilibrium constant for the reaction A B - C D is K when the initial concentration of A and B each is 0.1 mol/l under the similar conditions in an another experiment if the initial concentration of A and B are taken 2 and 3 mol/l respectively then the value of equilibrium constant will be? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about In an experiment the equilibrium constant for the reaction A B - C D is K when the initial concentration of A and B each is 0.1 mol/l under the similar conditions in an another experiment if the initial concentration of A and B are taken 2 and 3 mol/l respectively then the value of equilibrium constant will be? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for In an experiment the equilibrium constant for the reaction A B - C D is K when the initial concentration of A and B each is 0.1 mol/l under the similar conditions in an another experiment if the initial concentration of A and B are taken 2 and 3 mol/l respectively then the value of equilibrium constant will be?.
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