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26 February, 18:19

At a given temperature, 4.92 atm of Cl2 and 4.65 atm of Br2 are mixed and allowed to come to equilibrium. The equilibrium pressure of BrCl is found to be 1.597 atm. Calculate Kp for the reaction at this temperature. Cl2 (g) + Br2 (g) 2 BrCl (g). Give answer to 2 decimal places.

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  1. 26 February, 18:54
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    Kp = 0.16

    Explanation:

    Step 1: Data given

    Initial pressure of Cl2 = 4.92 atm

    Initial pressure of Br2 = 4.65 atm

    The equilibrium pressure of BrCl is found to be 1.597 atm

    Step 2: The balanced equation

    Cl2 (g) + Br2 (g) ⇔ 2 BrCl (g

    Step 3: The initial pressures

    pCl2 = 4.92 atm

    pBr2 = 4.65 atm

    pBrCl = 0 atm

    Step 4: The pressure at the equilibrium

    For 1 mol Cl2 we need 1 mol Br2 to produce 2 moles BrCl

    pCl2 = 4.92 - X atm

    pBr2 = 4.65 - Xatm

    pBrCl = 2X atm = 1.597 atm

    X = 1.597/2 = 0.7985 atm

    pCl2 = 4.92 - X atm = 4.92 - 0.7985 = 4.1215 atm

    pBr2 = 4.65 - Xatm = 3.8515 atm

    Step 5: Calculate Kp

    Kp = (BrCl) ² / (Cl2) * (Br2)

    Kp = 1.597² / (4.1215*3.8515)

    Kp = 0.16
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