### Chapter 16: Equilibrium Processes#### Be sure to answer all parts.Consider the following equilibrium process at 686°C:\[ \text{CO}_2 (g) + \text{H}_2 (g) \leftrightharpoons \text{CO} (g) + \text{H}_2\text{O} (g) \]The equilibrium concentrations of the reacting species are:\[ \left[ \text{CO} \right] = 0.0500 \, M, \quad \left[ \text{H}_2 \right] = 0.0420 \, M, \quad \left[ \text{CO}_2 \right] = 0.0900 \, M, \quad \left[ \text{H}_2\text{O} \right] = 0.0350 \, M \]**(a) Calculate \( K_c \) for the reaction at 686°C.**\[ \boxed{} \]**(b) If we add \(\text{CO}_2\) to increase its concentration to \(0.480 \, \text{mol/L}\), what will the concentrations of all the gases be when equilibrium is reestablished?****CO\(_2\):**\[ \boxed{\text{ } M} \]**H\(_2\):**\[ \boxed{\text{ } M} \]**CO:**\[ \boxed{\text{ } M} \]**H\(_2\)O:**\[ \boxed{\text{ } M} \]*Instructions: Enter your answers in the textboxes provided.*---#### Explanation of Graphs and Diagrams:*No graphs or diagrams are present on this page.*

In order to solve this question, law of mass action will be applied to calculate the value of Kc and…

Be sure to answer all parts. Consider the following equilibrium process at 686°C: CO;(g) + H2(g) = CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0500 M, (H2] = 0.0420 M, [CO2] = 0.0900 M, and [H,O] = 0.0350 M. %3D (a) Calculate K, for the reaction at 686°C. (b) If we add CO, to increase its concentration to 0.480 mol /L, what will the concentrations of all the gases be when equilibrium is reestablished?

Be sure to answer all parts. Consider the following equilibrium process at 686°C: CO;(g) + H2(g) = CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0500 M, (H2] = 0.0420 M, [CO2] = 0.0900 M, and [H,O] = 0.0350 M. %3D (a) Calculate K, for the reaction at 686°C. (b) If we add CO, to increase its concentration to 0.480 mol /L, what will the concentrations of all the gases be when equilibrium is reestablished?

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

### Chapter 16: Equilibrium Processes

#### Be sure to answer all parts.

Consider the following equilibrium process at 686°C:

\[ \text{CO}_2 (g) + \text{H}_2 (g) \leftrightharpoons \text{CO} (g) + \text{H}_2\text{O} (g) \]

The equilibrium concentrations of the reacting species are:

\[ \left[ \text{CO} \right] = 0.0500 \, M, \quad \left[ \text{H}_2 \right] = 0.0420 \, M, \quad \left[ \text{CO}_2 \right] = 0.0900 \, M, \quad \left[ \text{H}_2\text{O} \right] = 0.0350 \, M \]

**(a) Calculate \( K_c \) for the reaction at 686°C.**

\[ \boxed{} \]

**(b) If we add \(\text{CO}_2\) to increase its concentration to \(0.480 \, \text{mol/L}\), what will the concentrations of all the gases be when equilibrium is reestablished?**

**CO\(_2\):**

\[ \boxed{\text{ } M} \]

**H\(_2\):**

\[ \boxed{\text{ } M} \]

**CO:**

\[ \boxed{\text{ } M} \]

**H\(_2\)O:**

\[ \boxed{\text{ } M} \]

*Instructions: Enter your answers in the textboxes provided.*

---

#### Explanation of Graphs and Diagrams:

*No graphs or diagrams are present on this page.*

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