**Problem:**IBr decomposes according to the reaction at 150°C:\[ 2 \, \text{IBr (g)} \rightarrow \text{I}_2 \, \text{(g)} + \text{Br}_2 \, \text{(g)} \]If IBr is placed in a container at an initial pressure of 5.0 atm, what will be its equilibrium pressure at 150°C? \( K_p = 8.3 \times 10^{-3} \).**Explanation:**This problem involves the decomposition of iodine bromide (IBr) into iodine (I₂) and bromine (Br₂) gases at a temperature of 150°C. The initial pressure of IBr is 5.0 atm, and you need to calculate its equilibrium pressure using the equilibrium constant \( K_p \). **Key Concepts:**1. **Chemical Equilibrium:** - The condition in which the concentrations of the reactants and products do not change with time. 2. **Equilibrium Constant (\( K_p \)):** - It expresses the ratio of the concentrations of products to reactants at equilibrium, each raised to the power of their stoichiometric coefficients, but in terms of partial pressures for gases.3. **Reaction Stoichiometry:** - Requires understanding the mole ratios of reactants and products.The detailed understanding of these concepts will help students solve for the equilibrium pressure of the gases at the specified temperature.

Answered: Image /qna-images/answer/ef04274f-5f5e-4545-8f80-5cf6ecb04879.jpg

Answered: 2 IBr (g) = I2 (g) + Br2 (g) If IBr is…

2 IBr (g) = I2 (g) + Br2 (g) If IBr is placed in a container at an initial pressure of 5.0 atm, what will be its equilibrium pressure at 150ºC? Kp = 8.3 x 10-3

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

**Problem:**

IBr decomposes according to the reaction at 150°C:

\[ 2 \, \text{IBr (g)} \rightarrow \text{I}_2 \, \text{(g)} + \text{Br}_2 \, \text{(g)} \]

If IBr is placed in a container at an initial pressure of 5.0 atm, what will be its equilibrium pressure at 150°C? \( K_p = 8.3 \times 10^{-3} \).

**Explanation:**

This problem involves the decomposition of iodine bromide (IBr) into iodine (I₂) and bromine (Br₂) gases at a temperature of 150°C. The initial pressure of IBr is 5.0 atm, and you need to calculate its equilibrium pressure using the equilibrium constant \( K_p \).

**Key Concepts:**

1. **Chemical Equilibrium:**
- The condition in which the concentrations of the reactants and products do not change with time.

2. **Equilibrium Constant (\( K_p \)):**
- It expresses the ratio of the concentrations of products to reactants at equilibrium, each raised to the power of their stoichiometric coefficients, but in terms of partial pressures for gases.

3. **Reaction Stoichiometry:**
- Requires understanding the mole ratios of reactants and products.

The detailed understanding of these concepts will help students solve for the equilibrium pressure of the gases at the specified temperature.

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Step 1 To form the chemical equation to find partial pressure of each gas

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