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Test: Applications of Equilibrium Constants (July 21) - NEET MCQ


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10 Questions MCQ Test Daily Test for NEET Preparation - Test: Applications of Equilibrium Constants (July 21)

Test: Applications of Equilibrium Constants (July 21) for NEET 2024 is part of Daily Test for NEET Preparation preparation. The Test: Applications of Equilibrium Constants (July 21) questions and answers have been prepared according to the NEET exam syllabus.The Test: Applications of Equilibrium Constants (July 21) MCQs are made for NEET 2024 Exam. Find important definitions, questions, notes, meanings, examples, exercises, MCQs and online tests for Test: Applications of Equilibrium Constants (July 21) below.
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Test: Applications of Equilibrium Constants (July 21) - Question 1

What does the equilibrium constant (K) represent for a chemical reaction?

Detailed Solution for Test: Applications of Equilibrium Constants (July 21) - Question 1
The equilibrium constant (K) represents the ratio of product concentration to reactant concentration for a chemical reaction at equilibrium.
Test: Applications of Equilibrium Constants (July 21) - Question 2

Which of the following statements about equilibrium constants is true?

Detailed Solution for Test: Applications of Equilibrium Constants (July 21) - Question 2

The correct statement about equilibrium constants is:

     3. Equilibrium constants are different for the same reaction at different temperatures.

Here's a brief explanation of why the other statements are incorrect:

1. The equilibrium constant does not depend on the initial concentrations of reactants and products. It only depends on the ratio of the concentrations of products to reactants at equilibrium.

2. A catalyst does not change the value of the equilibrium constant. A catalyst only speeds up the rate at which equilibrium is reached.

4. Changes in concentration and pressure do not affect the equilibrium constant. However, changes in temperature do affect the equilibrium constant.

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Test: Applications of Equilibrium Constants (July 21) - Question 3

What is the relationship between the equilibrium constant Kc and the Gibbs free energy (?G) of a reaction?

Detailed Solution for Test: Applications of Equilibrium Constants (July 21) - Question 3
When ?G is greater than 0 and Qc is greater than Kc, it indicates a spontaneous reaction in the forward direction.
Test: Applications of Equilibrium Constants (July 21) - Question 4
What is the relationship between the forward and backward reaction rate constants at equilibrium?
Detailed Solution for Test: Applications of Equilibrium Constants (July 21) - Question 4
The forward and backward reaction rate constants are constant at a given temperature, leading to the establishment of the equilibrium constant.
Test: Applications of Equilibrium Constants (July 21) - Question 5
What happens to the equilibrium constant (K) of a reaction if the stoichiometry of the equilibrium reaction changes?
Detailed Solution for Test: Applications of Equilibrium Constants (July 21) - Question 5
If the stoichiometry of the equilibrium reaction changes, the equilibrium constant K remains the same as it is specific to the balanced equation at a given temperature.
Test: Applications of Equilibrium Constants (July 21) - Question 6
What happens to the equilibrium constant (K) when a catalyst is added to a reaction?
Detailed Solution for Test: Applications of Equilibrium Constants (July 21) - Question 6
The presence of a catalyst does not change the value of the equilibrium constant (K); it only affects the rate of the forward and backward reactions.
Test: Applications of Equilibrium Constants (July 21) - Question 7
How does the equilibrium constant (K) change with temperature for the same reversible reaction?
Detailed Solution for Test: Applications of Equilibrium Constants (July 21) - Question 7
The equilibrium constant (K) can have varying values at different temperatures for the same reversible reaction. It increases with increasing temperature.
Test: Applications of Equilibrium Constants (July 21) - Question 8
In the case of stepwise multiple equilibria leading to final products, how is the net equilibrium constant (K) determined?
Detailed Solution for Test: Applications of Equilibrium Constants (July 21) - Question 8
In the case of stepwise multiple equilibria leading to final products, the net equilibrium constant (K) is determined by taking the product of each stepwise equilibrium constant (K1 * K2 * K3).
Test: Applications of Equilibrium Constants (July 21) - Question 9
What unit is typically used for Kc, the equilibrium constant measured in terms of concentration?
Detailed Solution for Test: Applications of Equilibrium Constants (July 21) - Question 9
Kc is typically measured in moles per liter (mol/L) as it represents the concentration of products and reactants.
Test: Applications of Equilibrium Constants (July 21) - Question 10

How is the direction of a reaction determined using the equilibrium constant (K) and the reaction quotient (Q)?

Detailed Solution for Test: Applications of Equilibrium Constants (July 21) - Question 10

The correct answer is:

a) By comparing Q to K, where Q > K indicates a backward reaction, and Q < K indicates a forward reaction.

Explanation:

  • The reaction quotient Q is calculated using the concentrations of the reactants and products at any point during the reaction.
  • The equilibrium constant K is the value of Q when the reaction is at equilibrium.
  • If Q<K, the reaction will proceed in the forward direction to reach equilibrium (products are favored).
  • If Q>K, the reaction will proceed in the reverse direction to reach equilibrium (reactants are favored).
  • If Q=K, the reaction is at equilibrium, and there is no net change in the concentration of reactants and products.
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