The reaction CO(g) + H 2 O(g) ⇌ CO 2 (g) + H 2 (g) has ∆ H = -9.8 kcal/mol (-41 kJ/mol). Does the amount of H 2 in an equilibrium mixture increase or decrease when the temperature is decreased?

Hello everyone today. You're the falling problem. The entropy change for the falling reaction is negative. 54.97. Kill accounts promote what happens to the concentration of chlorine in the equilibrium mixture when the temperature is reduced. So according to a principle known as Les Chevaliers principle, a disturbance in the reaction. So a disturbance in the reaction causes the equilibrium to shift in that direction to relieve it, so it'll shift in that direction. And so the sense the entropy is given as negative entropy is negative. It is a product. So it can be tacked on the end on our product side as heat. So if the temperature was reduced meaning that heat was removed, then the equilibrium will shift towards the heat to increase the amount on the product side. So if our heat is reduced, the equilibrium shifts rightward shifts to the right and so if the reaction will shift to the right, which is the forward direction, we can say that we're going to have an increase in our products. So we're going to increase the amount of these two products here. So the concentration of chlorine is going to increase. And the answer choice that best reflects this is Angela is a concentration of chlorine equilibrium mixture increases when the temperature is reduced and with that we have answered the question overall, I hope it's 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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2:04 minutes

Problem 63

Textbook Question

The reaction CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g) has ∆H = -9.8 kcal/mol (-41 kJ/mol). Does the amount of H₂ in an equilibrium mixture increase or decrease when the temperature is decreased?

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Identify the type of reaction based on the given enthalpy change (∆H). Since ∆H = -9.8 kcal/mol, the reaction is exothermic, meaning it releases heat as a product.

Recall Le Châtelier's Principle, which states that if a system at equilibrium is subjected to a change in temperature, pressure, or concentration, the system will adjust to counteract that change and restore equilibrium.

Understand the effect of temperature on an exothermic reaction. Decreasing the temperature removes heat from the system. According to Le Châtelier's Principle, the equilibrium will shift to produce more heat, favoring the exothermic (forward) reaction.

Analyze the forward reaction: CO(g) + H2O(g) ⇌ CO2(g) + H2(g). Since the forward reaction produces H2 as a product, a shift toward the forward reaction will increase the amount of H2 in the equilibrium mixture.

Conclude that when the temperature is decreased, the equilibrium shifts toward the forward reaction, resulting in an increase in the amount of H2 in the equilibrium mixture.

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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 system will adjust to counteract the change and restore a new equilibrium. In the context of temperature changes, if the temperature is decreased, the equilibrium will shift in the direction that produces heat, which can affect the concentrations of reactants and products.

Exothermic Reactions

An exothermic reaction is one that releases heat, indicated by a negative enthalpy change (∆H). In this reaction, since ∆H = -9.8 kcal/mol, it means that heat is released when CO and H2O react to form CO2 and H2. Lowering the temperature favors the formation of products in exothermic reactions, as the system seeks to produce more heat.

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. Changes in temperature can alter the value of K, influencing the position of equilibrium. For exothermic reactions, a decrease in temperature typically increases K, favoring the formation of products, including H2.

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