Coal, which is primarily carbon, can be converted to natural gas, primarily CH 4 , by the exothermic reaction: C(s) + 2 H 2 (g) ⇌ CH 4 (g) Which disturbance will favor CH 4 at equilibrium? c. raising the temperature of the reaction mixture

Hello everyone. So in the problem, we're gonna go ahead and focus on this reaction right over here and saying which of the following will increase the formation of any age three. And we're gonna go ahead and assume that this is an exact thermic reaction. So, if the ration is X. Thermic, then he will be a product. So we'll say eat eggs. A thermic heat is product. In this case, let's go ahead and actually rewrite our equation. Then we'll have still N two gas plus three H two gas equilibrium arrows. And then we'll have to end age three, which is a gas. And we'll also have heat now. And so in a way we're saying that the we're increasing the temperature. If we increase the temperature, let's go ahead and write this at the bottom. I'm just gonna go ahead and move away from heat, which will cause equilibrium to shift to the right, which then makes more reactant. Now, for B, if we decrease the temperature, then we're moving towards the heat. If we meet towards the heat, we're gonna go ahead and have the equilibrium chipped to the left and because we're shifting to the left, then we're gonna go ahead and actually make more products. So we want to go ahead and increase the formation of NH three. NH 3 is a product. This will go ahead and actually make more products. Therefore our final answer is going to be be here where we decrease where we decrease the temperature Because we want more NH three a product. All right, thank you all so much for watching

Ch.15 - Chemical Equilibrium

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Tro 4th Edition

Ch.15 - Chemical Equilibrium

Problem 71c

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Chapter 15, Problem 71c

Coal, which is primarily carbon, can be converted to natural gas, primarily CH₄, by the exothermic reaction: C(s) + 2 H₂(g) ⇌ CH₄(g) Which disturbance will favor CH₄ at equilibrium? c. raising the temperature of the reaction mixture

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Identify the type of reaction: The given reaction C(s) + 2 H2(g) ⇌ CH4(g) is an exothermic reaction, meaning it releases heat.

Apply Le Chatelier's Principle: According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change, the system will adjust itself to counteract that change and restore a new equilibrium.

Analyze the effect of temperature: Increasing the temperature of an exothermic reaction adds heat to the system.

Predict the shift in equilibrium: Adding heat to an exothermic reaction will shift the equilibrium towards the reactants according to Le Chatelier's Principle.

Conclude the effect on CH4 production: Raising the temperature of the reaction mixture will not favor the production of CH4; instead, it will favor the formation of the reactants, C(s) and H2(g).

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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. This principle helps predict how a system at equilibrium will respond to changes in concentration, temperature, or pressure, favoring the formation of products or reactants.

Exothermic Reactions

An exothermic reaction is one that releases energy, usually in the form of heat, to the surroundings. In the given reaction, the formation of CH4 from carbon and hydrogen is exothermic, meaning that increasing the temperature will shift the equilibrium position to favor the reactants, as the system will try to absorb the added heat.

Equilibrium Constant (K)

The equilibrium constant (K) quantifies 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, increasing temperature typically decreases K, favoring reactants over products.

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Equilibrium Constant K

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Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. b. PCl₃(g) + Cl₂(g) ⇌ PCl₅(g) (volume is increased)

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Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. c. CaCO₃(s) ⇌ CaO(s) + CO₂(g) (volume is increased)

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This reaction is endothermic. C(s) + CO₂(g) ⇌ 2 CO(g) Predict the effect (shift right, shift left, or no effect) of increasing and decreasing the reaction temperature. How does the value of the equilibrium constant depend on temperature?

Coal, which is primarily carbon, can be converted to natural gas, primarily CH₄, by the exothermic reaction: C(s) + 2 H₂(g) ⇌ CH₄(g) Which disturbance will favor CH₄ at equilibrium? e. adding a catalyst to the reaction mixture

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Textbook Question

Coal can be used to generate hydrogen gas (a potential fuel) by the endothermic reaction: C(s) + H₂O(g) ⇌ CO(g) + H₂(g) If this reaction mixture is at equilibrium, predict whether each disturbance will result in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. e. adding a catalyst to the reaction mixture

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Coal, which is primarily carbon, can be converted to natural gas, primarily CH4, by the exothermic reaction: C(s) + 2 H2(g) ⇌ CH4(g) Which disturbance will favor CH4 at equilibrium? c. raising the temperature of the reaction mixture

Verified Solution

Key Concepts

Le Chatelier's Principle

Exothermic Reactions

Equilibrium Constant (K)

Coal, which is primarily carbon, can be converted to natural gas, primarily CH₄, by the exothermic reaction: C(s) + 2 H₂(g) ⇌ CH₄(g) Which disturbance will favor CH₄ at equilibrium? c. raising the temperature of the reaction mixture