For the equilibrium 2 IBr(g) ⇌ I2(g) + Br2(g), Kp = 8.5 * 10^-3 at 150 _x001F_C. If 0.025 atm of IBr is placed in a 2.0-L container, what is the partial pressure of all substances after equilibrium is reached?

Verified step by step guidance

Step 1: Write the expression for the equilibrium constant Kp for the reaction 2 IBr(g) ⇌ I2(g) + Br2(g). The expression is Kp = (P_{I2} * P_{Br2}) / (P_{IBr}^2), where P represents the partial pressures of the gases.

Step 2: Define the initial conditions. Initially, the partial pressure of IBr is 0.025 atm, and the partial pressures of I2 and Br2 are 0 atm since they are not present initially.

Step 3: Set up an ICE (Initial, Change, Equilibrium) table to track the changes in partial pressures. Let x be the change in pressure for I2 and Br2, and 2x for IBr since it dissociates into two moles of IBr for every mole of I2 and Br2 formed.

Step 4: Express the equilibrium partial pressures in terms of x. At equilibrium, P_{IBr} = 0.025 - 2x, P_{I2} = x, and P_{Br2} = x.

Step 5: Substitute the equilibrium partial pressures into the Kp expression and solve for x. Use the equation Kp = (x * x) / (0.025 - 2x)^2 = 8.5 * 10^-3 to find the value of x, which will allow you to calculate the equilibrium partial pressures of IBr, I2, and Br2.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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 state, the system is dynamic, meaning that reactions continue to occur, but there is no net change in the concentrations. The equilibrium constant (Kp) quantifies the ratio of the partial pressures of products to reactants at equilibrium, providing insight into the position of the equilibrium.

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. According to Dalton's Law, the total pressure of a gas mixture is the sum of the partial pressures of its individual gases. In equilibrium calculations, understanding how to calculate the partial pressures of each species is crucial for determining the equilibrium state of the system.

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 2 IBr(g) ⇌ I2(g) + Br2(g), Kp = (P_I2 * P_Br2) / (P_IBr^2). This constant helps predict the direction of the reaction and the concentrations of the substances at equilibrium, given initial conditions.

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