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25 October, 06:03

The equilibrium constant, Kp, for the following reaction is 9.52*10-2 at 350 K: CH4 (g) + CCl4 (g) 2CH2Cl2 (g) Calculate the equilibrium partial pressures of all species when CH4 and CCl4, each at an intitial partial pressure of 1.06 atm, are introduced into an evacuated vessel at 350 K. PCH4 = atm PCCl4 = atm PCH2Cl2 = atm

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  1. 25 October, 08:43
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    pCH4 = 0.9184 atm

    pCCl4 = 0.9184 atm

    pCH2Cl2 = 0.2832 atm

    Explanation:

    Step 1: Data given

    The equilibrium constant, Kp = 9.52 * 10^-2

    Temperature = 350 K

    Each have an initial pressure of 1.06 atm

    Step 2: The balanced equation

    CH4 (g) + CCl4 (g) ⇆ 2CH2Cl2 (g)

    Step 3: The pressure at the equilibrium

    pCH4 = 1.06 - X atm

    pCCl4 = 1.06 - X atm

    pCH2Cl2 = 2X

    Step 4: Calculate Kp

    Kp = (2X) ² / (1.06 - X) * (1.06 - X)

    9.52 * 10^-2 = 4X² / (1.06 - X) * (1.06 - X)

    X = 0.1416

    Step 5: Calculate the partial pressure

    pCH4 = 1.06 - 0.1416 = 0.9184 atm

    pCCl4 = 1.06 - 0.1416 = 0.9184 atm

    pCH2Cl2 = 2 * 0.1416 = 0.2832 atm

    Kp = (0.2832²) / (0.9184*0.9184)

    Kp = 9.52 * 10^-2

    pCH4 = 0.9184 atm

    pCCl4 = 0.9184 atm

    pCH2Cl2 = 0.2832 atm
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