bob asked in Science & MathematicsChemistry · 1 month ago

chemistry equilibrium?

The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K:

2CH2Cl2(g) CH4(g) + CCl4(g) 

Calculate the equilibrium partial pressures of all species when CH2Cl2(g) is introduced into an evacuated flask at a pressure of 0.847 atm at 350 K. 

PCH2Cl2= ____atm

PCH4= ____ atm

PCCl4= _____atm

1 Answer

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  • david
    Lv 7
    1 month ago
    Favorite Answer

    Kp  =  (P CH4)(P CCl4) / (P CH2Cl2)^2

    10.5  = (x/2)^2  /  (0.847 - x)^2  <<<<  round

    10.5 = (x/2)^2 / (0.847 )^2 <<<< solve

      x = 5.489  <<  not small  ,,,  must solve as a quadrtic

    10.5 = (x/2)^2 / (0.847 - x)^2

      10.5(0.847 - x)^2 =  x^2 /4

    42(0.847 - x)^2 = x^2

     x≈0.733776

    x≈1.00154   <<<  not possible .. x must be  < 0.847

      x = 0.734 atm  

      x/2 =  p CH4  =  p CCl4 = 0.367 atm

      P CH2Cl2 =  0.847 - x  =  0.113 atm

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