The following reaction is important in gold mining: 4 Au1s2 + 8 CN-1aq2 + O21g2 + 2 H2O1l2 ∆ 4 Au1CN22-1aq2 + 4 OH-1aq2For a reaction mixture at equilibrium, in which direction would the reaction go to reestablish equilibrium after each of the following changes? (a) Adding gold

검증된 단계별 안내

insert step 1> Identify the reaction and its components. The given reaction is: 4 Au_{(s)} + 8 CN^-_{(aq)} + O_2_{(g)} + 2 H_2O_{(l)} \(\rightarrow\) 4 Au(CN)_2^-_{(aq)} + 4 OH^-_{(aq)}.

insert step 2> Recognize that the reaction is at equilibrium, meaning the rate of the forward reaction equals the rate of the reverse reaction.

insert step 3> Apply Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.

insert step 4> Consider the effect of adding gold (Au) to the system. Since gold is a reactant, adding more gold will shift the equilibrium to the right to produce more products, in order to reduce the concentration of gold.

insert step 5> Conclude that the addition of gold will cause the reaction to shift towards the formation of more Au(CN)_2^- and OH^- ions, thus moving the equilibrium to the right.

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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 the direction in which the reaction will shift.

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 in understanding how changes in concentration affect the position of equilibrium.

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative concentrations of products and reactants at any point in a reaction, not just at equilibrium. By comparing Q to K, one can determine the direction in which the reaction will shift to reach equilibrium: if Q < K, the reaction shifts right (toward products), and if Q > K, it shifts left (toward reactants).