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?
a. adding more C to the reaction mixture b. adding more H₂ to the reaction mixture d. lowering the volume of the reaction mixture f. adding neon gas to the reaction mixture

검증된 단계별 안내

Identify the reaction and the type of reaction: The given reaction is C(s) + 2 H2(g) ⇌ CH4(g). This is a reversible reaction, and changes in conditions can shift the equilibrium position.

Understand 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 more H2: Adding more H2 increases the concentration of one of the reactants in the reaction mixture.

Predict the shift in equilibrium: According to Le Chatelier's Principle, increasing the concentration of H2 will shift the equilibrium to the right, towards the formation of more products.

Conclude the effect on CH4 production: Therefore, adding more H2 to the reaction mixture will favor the production of CH4 at equilibrium.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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, allowing us to determine which direction the reaction will favor.

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. For the reaction C(s) + 2 H2(g) ⇌ CH4(g), K can be calculated using the concentrations of CH4 and H2, providing insight into the extent of the reaction and the favorability of products versus reactants.

Exothermic Reactions

Exothermic reactions are chemical reactions that release energy, usually in the form of heat, to the surroundings. In the context of the given reaction, the conversion of carbon and hydrogen to methane (CH4) is exothermic, meaning that increasing the concentration of reactants like H2 can shift the equilibrium towards the production of more CH4, thereby favoring the formation of the product.