Answered

Discover the answers you need at Westonci.ca, a dynamic Q&A platform where knowledge is shared freely by a community of experts. Our Q&A platform offers a seamless experience for finding reliable answers from experts in various disciplines. Explore comprehensive solutions to your questions from knowledgeable professionals across various fields on our platform.

Consider the reaction [tex]$H_2(g) + I_2(g) \Leftrightarrow 2HI(g)$[/tex] with an equilibrium constant of 46.3 and a reaction quotient of 525. Which direction will the system shift?

A. The equilibrium will shift to the left to favor the reactants.
B. The equilibrium will shift to the right to favor the products.
C. The equilibrium will not shift in any direction.
D. The equilibrium will shift to the forward reaction.

Sagot :

GinnyAnswer
To address the question of which direction the given reaction will shift, we need to compare the reaction quotient ([tex]\(Q\)[/tex]) with the equilibrium constant ([tex]\(K_c\)[/tex]).

1. Identify the given values:
- Reaction Quotient ([tex]\(Q\)[/tex]): 525
- Equilibrium Constant ([tex]\(K_c\)[/tex]): 46.3

2. Understand the significance of [tex]\(Q\)[/tex] and [tex]\(K_c\)[/tex]:
- The reaction quotient ([tex]\(Q\)[/tex]) is a measure of the relative amounts of products and reactants at any point in time.
- The equilibrium constant ([tex]\(K_c\)[/tex]) is a measure of the relative amounts of products and reactants at equilibrium.

3. Comparison of [tex]\(Q\)[/tex] and [tex]\(K_c\)[/tex]:
- If [tex]\(Q < K_c\)[/tex], the reaction will shift to the right, towards the products, to reach equilibrium.
- If [tex]\(Q > K_c\)[/tex], the reaction will shift to the left, towards the reactants, to reach equilibrium.
- If [tex]\(Q = K_c\)[/tex], the reaction is already at equilibrium and will not shift in any direction.

4. Apply the given values:
- Here, we are given that [tex]\(Q = 525\)[/tex] and [tex]\(K_c = 46.3\)[/tex].

Since [tex]\(Q = 525\)[/tex] is greater than [tex]\(K_c = 46.3\)[/tex], the reaction quotient [tex]\(Q\)[/tex] indicates that there are more products relative to reactants than there would be at equilibrium. Therefore, to reach equilibrium, the system needs to reduce the excess products and increase the reactants.

5. Determine the direction of the shift:
- Because [tex]\(Q > K_c\)[/tex], the equilibrium will shift to the left to favor the reactants.

Therefore, the correct answer is:
The equilibrium will shift to the left to favor the reactants.
We appreciate your time on our site. Don't hesitate to return whenever you have more questions or need further clarification. Thanks for stopping by. We strive to provide the best answers for all your questions. See you again soon. Find reliable answers at Westonci.ca. Visit us again for the latest updates and expert advice.