Consider the reaction: A(g) ⇌ 2B(g). Find the equilibrium partial pressures of A and B for each value of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions. a. Kp = 1.0 b. Kp = 1.0 × 10^-4 c. Kp = 1.0 × 10^5.

Name: Chemistry: A Molecular Approach
Author: Tro
ISBN: 9780137832217

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주요 개념

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

Chemical 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 case, the reaction A(g) ⇌ 2B(g) reaches a state where the partial pressures of A and B remain unchanged over time. Understanding this concept is crucial for analyzing how changes in conditions affect the equilibrium position and the concentrations of the species involved.

Equilibrium Constant (Kp)

The equilibrium constant, Kp, is a dimensionless value that expresses the ratio of the partial pressures of products to reactants at equilibrium, raised to the power of their stoichiometric coefficients. For the reaction A(g) ⇌ 2B(g), Kp is calculated as Kp = (P_B^2) / (P_A). Different values of Kp indicate the extent to which the reaction favors products or reactants, which is essential for determining the equilibrium partial pressures in this scenario.

ICE Table (Initial, Change, Equilibrium)

An ICE table is a systematic way to organize the initial concentrations (or partial pressures), the changes that occur as the system reaches equilibrium, and the equilibrium concentrations. For the given reaction, the initial pressures of A and B, the changes in their pressures as the reaction proceeds, and the final equilibrium pressures can be calculated using this table. This method simplifies the process of solving for unknowns in equilibrium problems.