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

검증된 단계별 안내

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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주요 개념

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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.

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