Question

At 1000 Kelvin, the value of Kp = 4.8 for the following reaction: 2 BrCl (g) ⇌ Br2 (g) + Cl2 (g) If at equilibrium, it was determined that BrCl = 0.15 atm and Cl₂ = 0.33 atm, Options: Option 1: The partial pressure of Br2 (g) at equilibrium is 0.33 atm. Option 2: The partial pressure of Br2 (g) at equilibrium is 0.075 atm. Option 3: The partial pressure of Br2 (g) at equilibrium is 0.24 atm. Option 4: The partial pressure of Br2 (g) at equilibrium is 0.15 atm.

Answer 1

The partial pressure of Br2 at equilibrium can be calculated by substituting the given values into the expression for the equilibrium constant of the reaction, Kp = [Br2][Cl2]/[BrCl]^2, and solving for [Br2].

Step-by-step explanation:

The question is about the calculation of equilibrium partial pressures in a chemical reaction involving gases. In the given reaction, 2 BrCl (g) ⇌ Br2 (g) + Cl2 (g), with Kp = 4.8 at 1000 Kelvin, equilibrium concentrations of BrCl and Cl2 are given as 0.15 atm and 0.33 atm, respectively. Using the expression for the equilibrium constant for this reaction, i.e., Kp = [Br2][Cl2]/[BrCl]^2, we can solve for the unknown equilibrium partial pressure of Br2 (P_{Br2}). Since Kp, P_{BrCl}, and P_{Cl2} are known, just substitute these values in the aforementioned equilibrium constant expression and solve for P_{Br2}.

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