A platinum catalyst is used in automobile catalytic convert- ers to hasten the oxidation of carbon monoxide: 2 CO1g2 + O 1g2 ∆Pt 2 CO 1g2 ΔH° = - 566 kJ Suppose that you have a reaction vessel containing an equilibrium mixture of CO1g2, O21g2, and CO21g2. Under the following conditions, will the amount of CO increase, decrease, or remain the same? (e) The pressure is increased by adding O2 gas.

검증된 단계별 안내

Identify the reaction: \(2 \text{CO}(g) + \text{O}_2(g) \xrightarrow{\text{Pt}} 2 \text{CO}_2(g)\).

Recognize that the reaction is exothermic with \(\Delta H^\circ = -566 \text{kJ}\).

Apply Le Chatelier's Principle: Increasing the pressure by adding \(\text{O}_2\) will shift the equilibrium to the side with fewer moles of gas.

Count the moles of gas on each side: Reactants have 3 moles (2 CO + 1 O2), and products have 2 moles (2 CO2).

Conclude that adding \(\text{O}_2\) increases pressure, shifting equilibrium to the right, decreasing \(\text{CO}\).

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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 system will adjust to counteract the change and restore a new equilibrium. In the context of chemical reactions, this means that if the concentration of a reactant or product is altered, the equilibrium will shift in a direction that reduces the effect of that change.

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. It provides insight into the extent of the reaction and helps predict how changes in concentration, pressure, or temperature will affect the position of equilibrium.

Effect of Pressure on Gaseous Reactions

In gaseous reactions, changes in pressure can influence the position of equilibrium, particularly when the number of moles of gas differs between reactants and products. Increasing the pressure will favor the side of the reaction with fewer moles of gas, while decreasing pressure favors the side with more moles. This principle is crucial for predicting how the addition of gases, like O2, will affect the concentrations of CO and other species in the reaction.