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3 April, 15:16

Ammonium carbamate (NH2COONH4) is a salt of carbamic acid that is found in the blood and urine of mammals. At 202°C, Kc = 0.008 for the following equilibrium: If 6.82 g of NH2COONH4 is put into a 0.5-L evacuated container, what is the total pressure (in atm) at equilibrium? Enter a number to 2 decimal places.

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  1. 3 April, 15:34
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    P (total) = 46.08 atm

    Explanation:

    Given dа ta:

    Mass of NH₂COONH₄ = 6.8 g

    Kc = 0.008

    Temperature = 202°C = 202+273 = 475 K

    Total pressure at equilibrium = ?

    Solution:

    Equilibrium equation:

    NH₂COONH₄ ⇄ 2NH₃ + CO₂

    Formula:

    Kp = Kc (RT) ³

    Kp = 0.008 (0.0821 atm. L/mol. K) ³ (475K) ³

    Kp = 471.56

    NH₃ CO₂

    Initial concentration 0 0

    Change in concentration 2x x

    equilibrium concentration 2x x

    AS

    471.56 = 2x (x)

    471.56 = 2x²

    x² = 471.56 / 2

    x² = 235.78

    x = 15.36

    Pressure of ammonia = 2x = 2 (15.36) = 30.72 atm

    Pressure of carbon dioxide = x = 15.36 atm

    Total pressure:

    P (total) = P (NH₃) + P (CO₂)

    P (total) = 30.72 atm + 15.36 atm

    P (total) = 46.08 atm
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