For the reaction A2 + 2B ∆ 2 AB, the rate of the for- ward reaction is 18 M/s and the rate of the reverse reaction is 12 M/s. The reaction is not at equilibrium. Will the reaction pro- ceed in the forward or reverse direction to attain equilibrium?

검증된 단계별 안내

Identify the rates of the forward and reverse reactions. The rate of the forward reaction is given as 18 M/s, and the rate of the reverse reaction is 12 M/s.

Understand that at equilibrium, the rate of the forward reaction equals the rate of the reverse reaction.

Compare the given rates: since the rate of the forward reaction (18 M/s) is greater than the rate of the reverse reaction (12 M/s), the reaction system is producing AB faster than it is being converted back to A2 and B.

Determine the direction needed to reach equilibrium: To achieve equilibrium, the system needs to slow down the forward reaction or speed up the reverse reaction until both rates are equal.

Conclude that the reaction will proceed in the forward direction to increase the concentration of products (AB), which will eventually increase the rate of the reverse reaction and help attain equilibrium.

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주요 개념

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

Reaction Rates

Reaction rates refer to the speed at which reactants are converted into products in a chemical reaction. In this case, the forward reaction rate is 18 M/s, while the reverse reaction rate is 12 M/s. Understanding these rates is crucial for determining the direction in which the reaction will proceed to reach equilibrium.

Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In this scenario, since the forward reaction rate (18 M/s) is greater than the reverse reaction rate (12 M/s), the system is not at equilibrium and will shift towards the formation of more products to achieve balance.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed, it will adjust to counteract the disturbance and restore a new equilibrium. In this case, since the forward reaction is faster, the system will favor the forward direction to increase the concentration of products (AB) until the rates of both reactions equalize.