### Chemical Equilibrium Problems#### 3. Reaction Analysis**Reaction:** \[ \text{Br}_2(g) + \text{Cl}_2(g) \rightleftharpoons 2 \text{BrCl}(g) \]**Equilibrium Constant (K\_p):** \[ K\_p = 1.11 \times 10^{-4} \, \text{at 150 K} \]**Initial Conditions:** - Partial pressure of Br\(_2\) = 0.993 atm- Partial pressure of Cl\(_2\) = 0.967 atm**Task:** Calculate the equilibrium partial pressures of Br\(_2\), Cl\(_2\), and BrCl at 150 K.#### 4. Reaction Analysis**Reaction:** \[ \text{CO}(g) + \text{H}_2\text{O}(g) \rightleftharpoons \text{CO}_2(g) + \text{H}_2(g) \]**Equilibrium Constant (K\_p):** \[ K\_p = 0.0611 \, \text{at 2000 K} \]**Initial Conditions:** - Partial pressure of CO = 1.768 atm- Partial pressure of H\(_2\)O = 2.324 atm**Task:** Calculate the equilibrium partial pressures of CO, H\(_2\)O, CO\(_2\), and H\(_2\) at 2000 K.---**Instructions for Solving the Problems:**1. **Write the expression for K\_p:** Based on the reaction equations, write the expression for K\_p using the ratio of products to reactants, each raised to the power of their coefficients in the balanced equation.2. **Use an ICE Table:** Set up an ICE (Initial, Change, Equilibrium) table to help visualize changes in partial pressures from initial conditions to equilibrium.3. **Solve for Changes (x):** Use algebraic methods to solve for changes in pressure (\(x\)) and determine the equilibrium pressures.4. **Calculate Equilibrium Pressures:** Use \(x\) to find the equilibrium pressures for each substance.5. **Verify Results:** Ensure your calculated pressures satisfy the K\_p expression.

We will use the equilibrium constant Kp to calculate the equilibrium partial pressure. We will…

3. Consider the reaction Br2 (g) + Cl2 (9) 2 BrCl (g) Kp = 1.11 x 10 at 150 K. A reaction mixture initially contains a Br₂ partial pressure of 0.993 atm and a Cl₂ partial pressure of 0.967 atm at 150 K. Calculate the equilibrium partial pressure of each reactant and product. 4. Consider the reaction CO (g) + H₂O (g) CO₂ (g) + H₂ (g) A reaction mixture initially contains a CO partial pressure of 1.768 atm and a H₂O partial pressure of 2.324 atm at 2000 K. Calculate the equilibrium partial pressures of each reactant and product. p= 0.0611 at 2000K.

3. Consider the reaction Br2 (g) + Cl2 (9) 2 BrCl (g) Kp = 1.11 x 10 at 150 K. A reaction mixture initially contains a Br₂ partial pressure of 0.993 atm and a Cl₂ partial pressure of 0.967 atm at 150 K. Calculate the equilibrium partial pressure of each reactant and product. 4. Consider the reaction CO (g) + H₂O (g) CO₂ (g) + H₂ (g) A reaction mixture initially contains a CO partial pressure of 1.768 atm and a H₂O partial pressure of 2.324 atm at 2000 K. Calculate the equilibrium partial pressures of each reactant and product. p= 0.0611 at 2000K.

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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