Assume that the following reaction is at equilibrium at 100 oC CH4(g) + H2O(g) <-->3 H2(g) + CO(g) ΔH = 131.3 kJ Which one of the following changes will cause the reaction to shift to the right? a. Increasing the pressure. b. Increasing the temperature. c. Decreasing the methane gas concentration d. Increasing the carbon monoxide concentration. e. Decreasing the volume of the container.
Assume that the following reaction is at equilibrium at 100 oC CH4(g) + H2O(g) <-->3 H2(g) + CO(g) ΔH = 131.3 kJ Which one of the following changes will cause the reaction to shift to the right? a. Increasing the pressure. b. Increasing the temperature. c. Decreasing the methane gas concentration d. Increasing the carbon monoxide concentration. e. Decreasing the volume of the container.
Chemistry
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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
Assume that the following reaction is at equilibrium at 100 oC
CH4(g) + H2O(g) <-->3 H2(g) + CO(g) ΔH = 131.3 kJ
Which one of the following changes will cause the reaction to shift to the right?
a. |
Increasing the pressure.
|
|
b. |
Increasing the temperature.
|
|
c. |
Decreasing the methane gas concentration
|
|
d. |
Increasing the carbon monoxide concentration.
|
|
e. |
Decreasing the volume of the container.
|
Expert Solution
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Step 1
As we know that, according to Le-Chatelier's principle, the equilibrium will shift in that direction which minimizes the change.
On increasing the pressure reaction moves towards the reactant side.
So, it would shift reaction towards left.
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