Nitric oxide (NO) reacts readily with chlorine gas as follows: 2 NO(𝑔) + Cl₂(𝑔) ⇌ 2 NOCl(𝑔) At 700 K, the equilibrium constant 𝐾_𝑝 for this reaction is 0.26. For each of the following mixtures at this temperature, indicate whether the mixture is at equilibrium, or, if not, whether it needs to produce more products or reactants to reach equilibrium. (b) 𝑃_NO= 0.12atm, 𝑃_Cl2= 0.10atm, 𝑃_NOCl= 0.050atm

검증된 단계별 안내

Calculate the reaction quotient, Qp, using the formula: Qp = (P_NOCl)^2 / (P_NO)^2 * (P_Cl2).

Substitute the given partial pressures into the Qp expression: P_NO = 0.12 atm, P_Cl2 = 0.10 atm, P_NOCl = 0.050 atm.

Compare the calculated Qp value with the given equilibrium constant Kp = 0.26.

If Qp = Kp, the system is at equilibrium. If Qp < Kp, the reaction will proceed in the forward direction to produce more products. If Qp > Kp, the reaction will proceed in the reverse direction to produce more reactants.

Based on the comparison, determine whether the mixture is at equilibrium or if it needs to shift to reach equilibrium.

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주요 개념

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

Equilibrium Constant (Kp)

The equilibrium constant, Kp, quantifies the ratio of the partial pressures of products to reactants at equilibrium for a given reaction. For the reaction 2 NO(g) + Cl2(g) ⇌ 2 NOCl(g), Kp is calculated as (P_NOCl^2) / (P_NO^2 * P_Cl2). A Kp value of 0.26 indicates that at equilibrium, the concentration of products is relatively low compared to reactants, guiding predictions about the direction of the reaction.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed by changes in concentration, pressure, or temperature, the system will adjust to counteract the disturbance and restore a new equilibrium. In this context, if the partial pressures of NO, Cl2, or NOCl are altered, the reaction will shift towards the side that reduces the effect of the change, either producing more products or reactants.

Reaction Quotient (Q)

The reaction quotient, Q, is calculated using the same formula as Kp but with the current partial pressures of the reactants and products. By comparing Q to Kp, one can determine the direction in which the reaction will proceed to reach equilibrium. If Q < Kp, the reaction will shift to the right (producing more products), while if Q > Kp, it will shift to the left (producing more reactants).