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17 August, 07:52

gaseous h2 and br2 are added to an evacuated 1.15L container kept at 298K. The intial partial pressurre of H2 (g) is 0.782 atm and that of Br2 (g) is 0.493 atm. Find the partial pressures of HBr when the system reaches equilibrium

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  1. 17 August, 08:18
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    The partial pressures of HBr when the system reaches equilibrium is 2.4 X 10⁻¹¹ atm

    Explanation:

    H₂ + Br₂ ⇒ 2HBr

    PH₂ = 0.782atm

    PBr₂ = 0.493atm

    Kp = (PHBr) ² / (PH₂) (PBr₂) = 1.4 X 10⁻²¹

    At equilibrium:

    Let 2x = pressure of HBr

    PH₂ = 0.782 - x

    PBr₂ = 0.493 - x

    Kp = (2x) ^2 / (0.782-x) (0.493-x)

    Now, because Kp is very small, x will be very small compared to 0.782 and 0.493.

    Then,

    Kp = 1.4X10⁻²¹ = (4x²) / (0.782) (0.493)

    x = 1.2X10⁻¹¹

    PHBr = 2x = 2.4 X 10⁻¹¹ atm

    Therefore, the partial pressures of HBr when the system reaches equilibrium is 2.4 X 10⁻¹¹ atm
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