**Chemical Equilibrium and Equilibrium Constant (Kp): Understanding Reversible Reactions**In a given chemical reaction, equilibrium involves the balance between the forward and reverse reactions.**Problem Statement:**For the reaction:\[ \text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g) \]The equilibrium constant, \( K_p \), is given as 1.84 at a certain temperature. Determine the value of \( K_p \) for the reverse reaction:\[ \text{PCl}_3(g) + \text{Cl}_2(g) \rightleftharpoons \text{PCl}_5(g) \]**Solution:**In equilibrium chemistry, the equilibrium constant for the reverse reaction is simply the reciprocal of the equilibrium constant for the forward reaction.Given:\[ K_p (\text{forward}) = 1.84 \]Therefore, the equilibrium constant for the reverse reaction is:\[ K_p (\text{reverse}) = \frac{1}{K_p (\text{forward})} = \frac{1}{1.84} \]This box indicates the answer, which confirms that the calculated value of \( K_p (\text{reverse}) \) is 1.84.Understanding the relationship between forward and reverse reactions is essential for equilibrium calculations in chemistry.

Answered: Image /qna-images/answer/874cc68c-c14f-458b-b1dd-ee37ab8ec9fc.jpg

Answered: PCI5(g) → PCI3(g) + Cl2(g) has Kp =…

PCI5(g) → PCI3(g) + Cl2(g) has Kp = 1.84 at a given temperature. What is the value of Kp for the reaction PCI3(g) + Cl2(g)<>PCI5(g) at the same temperature?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

**Chemical Equilibrium and Equilibrium Constant (Kp): Understanding Reversible Reactions**

In a given chemical reaction, equilibrium involves the balance between the forward and reverse reactions.

**Problem Statement:**

For the reaction:

\[ \text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g) \]

The equilibrium constant, \( K_p \), is given as 1.84 at a certain temperature. Determine the value of \( K_p \) for the reverse reaction:

\[ \text{PCl}_3(g) + \text{Cl}_2(g) \rightleftharpoons \text{PCl}_5(g) \]

**Solution:**

In equilibrium chemistry, the equilibrium constant for the reverse reaction is simply the reciprocal of the equilibrium constant for the forward reaction.

Given:

\[ K_p (\text{forward}) = 1.84 \]

Therefore, the equilibrium constant for the reverse reaction is:

\[ K_p (\text{reverse}) = \frac{1}{K_p (\text{forward})} = \frac{1}{1.84} \]

This box indicates the answer, which confirms that the calculated value of \( K_p (\text{reverse}) \) is 1.84.

Understanding the relationship between forward and reverse reactions is essential for equilibrium calculations in chemistry.

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