# Using Le Chatelier's Principle to Predict the Result of Changing Conditions in a Reaction## Reaction DetailsMethane and water react to form hydrogen and carbon monoxide, as shown in the chemical equation:\[ \text{CH}_4(g) + \text{H}_2\text{O}(g) \rightarrow 3\text{H}_2(g) + \text{CO}(g) \]The reaction is endothermic. Suppose a mixture of CH₄, H₂O, H₂, and CO has reached equilibrium in a closed reaction vessel. This exercise is to predict how certain changes will affect the composition of the mixture and the direction of equilibrium.## Table of Perturbations| Perturbation | Change in Composition | Shift in Equilibrium ||-----------------------------------|-----------------------------|----------------------|| **The temperature is raised.** | The pressure of CO will: | ○ to the right || | [ **?** ] | ○ to the left || | | ○ (none) || **The temperature is lowered.** | The pressure of CH₄ will: | ○ to the right || | [go up, go down, not change] | ○ to the left || | | ○ (none) |### Dropdown Options Explanation:- **Change in Composition Drop-down:** For the change in pressure of CO when the temperature is raised, a dropdown is provided with options to choose how it will be affected: "go up," "go down," or "not change." - **Shift in Equilibrium Choices:** For each perturbation, there are radio button options to select whether the equilibrium shifts to the right, shifts to the left, or remains unchanged.### Concepts:- **Endothermic Reaction:** An increase in temperature generally favors the endothermic direction (right shift for this reaction).- **Le Chatelier's Principle:** States that if an external change is applied to a system at equilibrium, the system adjusts to partially offset the effect of the change. In this case, temperature changes will affect the reaction direction.In this exercise, you must select the correct outcomes based on the principles of chemical equilibrium.

Given,The reaction:CH4 (g) + H2O (g) 3 H2 (g) + CO (g) ( endothermic reaction )…

Methane and water react to form hydrogen and carbon monoxide, like this: CH₂(g) + H₂O(g) → 3H₂(g) + CO(g) The reaction is endothermic. Suppose a mixture of CH4, H₂O, H₂ and CO has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition The temperature is raised. The pressure of CO will ? The temperature is lowered. The pressure of CH4 will? go up. go down. not change. shift in equilibrium O to the right to the left O (none) to the right to the left O (none) X

Methane and water react to form hydrogen and carbon monoxide, like this: CH₂(g) + H₂O(g) → 3H₂(g) + CO(g) The reaction is endothermic. Suppose a mixture of CH4, H₂O, H₂ and CO has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition The temperature is raised. The pressure of CO will ? The temperature is lowered. The pressure of CH4 will? go up. go down. not change. shift in equilibrium O to the right to the left O (none) to the right to the left O (none) X

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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# Using Le Chatelier's Principle to Predict the Result of Changing Conditions in a Reaction

## Reaction Details

Methane and water react to form hydrogen and carbon monoxide, as shown in the chemical equation:

\[ \text{CH}_4(g) + \text{H}_2\text{O}(g) \rightarrow 3\text{H}_2(g) + \text{CO}(g) \]

The reaction is endothermic. Suppose a mixture of CH₄, H₂O, H₂, and CO has reached equilibrium in a closed reaction vessel. This exercise is to predict how certain changes will affect the composition of the mixture and the direction of equilibrium.

## Table of Perturbations

| Perturbation | Change in Composition | Shift in Equilibrium |
|-----------------------------------|-----------------------------|----------------------|
| **The temperature is raised.** | The pressure of CO will: | ○ to the right |
| | [ **?** ] | ○ to the left |
| | | ○ (none) |
| **The temperature is lowered.** | The pressure of CH₄ will: | ○ to the right |
| | [go up, go down, not change] | ○ to the left |
| | | ○ (none) |

### Dropdown Options Explanation:

- **Change in Composition Drop-down:** For the change in pressure of CO when the temperature is raised, a dropdown is provided with options to choose how it will be affected: "go up," "go down," or "not change."

- **Shift in Equilibrium Choices:** For each perturbation, there are radio button options to select whether the equilibrium shifts to the right, shifts to the left, or remains unchanged.

### Concepts:

- **Endothermic Reaction:** An increase in temperature generally favors the endothermic direction (right shift for this reaction).
- **Le Chatelier's Principle:** States that if an external change is applied to a system at equilibrium, the system adjusts to partially offset the effect of the change. In this case, temperature changes will affect the reaction direction.

In this exercise, you must select the correct outcomes based on the principles of chemical equilibrium.

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