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1 January, 00:13

The equilibrium constant at 35 0 K for the reaction Br2 (g) I2 (g) 2IBr (g) has a value of 322. Bromine at an initial pressure of 0. 0500 atm is mixed with iodine at an initial partial pressure of 0. 0400 atm and held at 35 0 K until equilibrium is reached. Calculate the equilibrium pressure of each of the gases.

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  1. 1 January, 00:31
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    Partial pressure of Br2 = 0.01158 atm

    Partial pressure of I2 = 0.00158 atm

    Partial pressure of IBr = 0.07684 atm

    Explanation:

    Step 1: Data given

    Temperature = 350 K

    K = 322

    Initial partial pressure of bromine = 0.0500 atm

    Initial partial pressure of iodine = 0.0400 atm

    Step 2: The balanced equation

    Br2 (g) + I2 ⇆ 2IBr (g)

    Step 3: The initial pressures

    pBr2 = 0.0500 atm

    pI2 = 0.0400 atm

    pIBr = 0 atm

    Step 3: The pressure ate the equilibrium

    pBr2 = 0.0500 - X atm

    pI2 = 0.0400 - X atm

    pIBr = 2X atm

    Step 4: Define K

    K = (pIBr) ² / (pBr2) * (pI2)

    Step 5: Calculate X

    322 = (2X) ² / (0.0500-X) (0.0400-X)

    X = 0.03842

    pBr2 = 0.0500 - 0.03842 = 0.01158 atm

    pI2 = 0.0400 - 0.03842 = 0.00158 atm

    pIBr = 2*0.03842 = 0.07684 atm
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