What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen? C(s) + 2 H 2 (g) ⇌ CH 4 (g) ∆ H = -18 kcal/mol (-75kJ/mol) b. Increasing pressure by decreasing volume

Hello everyone today. We have the following problem. How does increasing the pressure, which is the same as decreasing the volume shift the equilibrium of the reaction of uranium with flooring gas? Well, according to a principle known as the chandeliers principle, they shot the ears principal, increasing the pressure, which is the same thing as decreasing the volume shifts the reaction. So shifts the reaction to the side with less gaseous moles. So if you look at the equation here, our reactant, our reactions, we have three moles of our flooring gas, we have three moles of gas and if you look on our products sign, We have simply one mole of gas. And so the products has the least amount of gaseous moles. So therefore we can conclude that increasing the pressure of the reaction which is the same as decreasing the volume, will shift the equilibrium forward, favoring the formation of products. And with that we have solved the problem overall, I hope this helped, and until next time.

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7. Energy, Rate and Equilibrium

Le Chatelier's Principle

GOB Chemistry

7. Energy, Rate and Equilibrium

Le Chatelier's Principle

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Problem 16b

Textbook Question

What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?
C(s) + 2 H₂(g) ⇌ CH₄(g) ∆H = -18 kcal/mol (-75kJ/mol)
b. Increasing pressure by decreasing volume

Verified step by step guidance

Identify the type of reaction: The reaction involves gases (H₂ and CH₄) and a solid (C). Since solids do not affect equilibrium, focus on the gaseous species. The reaction converts 2 moles of H₂ gas into 1 mole of CH₄ gas, resulting in a net decrease in the number of gas moles.

Understand the effect of pressure changes on equilibrium: According to Le Châtelier's Principle, if the pressure is increased (by decreasing volume), the equilibrium will shift to the side with fewer gas moles to counteract the change.

Apply the principle to this reaction: The reactant side has 2 moles of H₂ gas, while the product side has 1 mole of CH₄ gas. Since the product side has fewer gas moles, the equilibrium will shift toward the product side (CH₄) to reduce the pressure.

Relate the shift to the reaction's enthalpy: While the enthalpy change (∆H = -18 kcal/mol) indicates the reaction is exothermic, this does not directly affect the shift caused by pressure changes. The shift is determined solely by the number of gas moles in this case.

Conclude the effect: Increasing pressure by decreasing volume will shift the equilibrium position toward the product side, favoring the formation of CH₄ gas.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. In the context of the given reaction, increasing pressure by decreasing volume will favor the side of the reaction with fewer moles of gas, which can help predict how the equilibrium will shift.

Mole Ratio in Gaseous Reactions

In the reaction C(s) + 2 H2(g) ⇌ CH4(g), there are two moles of hydrogen gas on the reactant side and one mole of methane gas on the product side. Understanding the mole ratio is crucial because changes in pressure affect the gaseous components, and the equilibrium will shift towards the side with fewer moles of gas to reduce the pressure.

Effect of Pressure on Equilibrium

The effect of pressure on equilibrium is significant in reactions involving gases. Increasing pressure typically shifts the equilibrium towards the side with fewer gas molecules. In this case, since the product side has one mole of gas (CH4) compared to two moles of gas (H2) on the reactant side, increasing pressure will shift the equilibrium to the right, favoring the production of methane.

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