Assume that the following reaction is at equilibrium at 100 oCCH4(g) + H2O(g) <-->3 H2(g) + CO(g) ΔH = 131.3 kJWhich 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.

Answered: Assume that the following reaction is…

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

Assume that the following reaction is at equilibrium at 100 ^oC

CH₄_(g) + H₂O_(g) <-->3 H_2(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

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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