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? e. adding a catalyst to the reaction mixture

Hi everyone here we have a question asking which of the following will not affect the concentration of ammonia in the following exit thermic reaction at equilibrium nitrogen gash plus three hydrogen gasses forms to ammonia gasses. So a increasing temperature will shift away from added heat will decrease the concentration of ammonia B, decreasing volume, four moles of gas reacting and two moles of gas product will increase pressure. Will shift reaction to less gas moles will increase ammonia, see increasing pressure, increasing pressure will also shift the reaction to less gas animals will increase ammonia D adding a catalyst to the reaction mixture catalyst, increased rate of reaction but not the concentration of the product of reaction, so it will not change in the amount. So our answer here is the thank you for watching. Bye.

Ch.15 - Chemical Equilibrium

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Ch.15 - Chemical Equilibrium

Problem 71e

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Chapter 15, Problem 71e

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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Understand the role of a catalyst: A catalyst speeds up the rate of a reaction by lowering the activation energy. It does this without being consumed in the reaction.

Identify the reaction type: The given reaction C(s) + 2 H2(g) ⇌ CH4(g) is an equilibrium reaction, where reactants and products reach a state where their concentrations remain constant over time.

Recall Le Chatelier's Principle: This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

Analyze the effect of adding a catalyst: Adding a catalyst to an equilibrium reaction affects the rates of both the forward and reverse reactions equally. Therefore, it helps the system reach equilibrium faster but does not change the position of equilibrium.

Conclude the effect on CH4 production: Since adding a catalyst does not change the concentrations of reactants or products at equilibrium, it does not favor the production of CH4 specifically.

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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, pressure, or temperature, ultimately favoring the formation of products or reactants.

Exothermic Reactions

An exothermic reaction is a chemical reaction that releases energy in the form of heat. In the context of the given reaction, the conversion of carbon and hydrogen to methane (CH4) releases energy, which can influence the equilibrium position. Understanding whether a reaction is exothermic or endothermic is crucial for predicting how changes in temperature will affect the equilibrium.

Catalysts and Equilibrium

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. While catalysts do not affect the position of equilibrium, they help the system reach equilibrium faster. In the context of the question, adding a catalyst would not favor the formation of CH4 at equilibrium, as it does not shift the equilibrium position but merely accelerates the reaction rate.

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Related Practice

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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Textbook Question

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? c. raising the temperature of 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

Carbon monoxide replaces oxygen in oxygenated hemoglobin according to the reaction: HbO₂(aq) + CO(aq) ⇌ HbCO(aq) + O₂(aq) a. Use the reactions and associated equilibrium constants at body temperature given here to find the equilibrium constant for the reaction just shown. Hb(aq) + O₂(aq) ⇌ HbO₂(aq) K_c = 1.8 Hb(aq) + CO(aq) ⇌ HbCO(aq) K_c = 306

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Open Question

The reaction CO2(g) + C(s) ⇌ 2 CO(g) has Kp = 5.78 at 1200 K. a. Calculate the total pressure at equilibrium when 4.45 g of CO2 is introduced into a 10.0-L container and heated to 1200 K in the presence of 2.00 g of graphite. b. Repeat the calculation of part a in the presence of 0.50 g of graphite.

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

Verified Solution

Key Concepts

Le Chatelier's Principle

Exothermic Reactions

Catalysts and Equilibrium

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