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For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌...

For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌ COCl2 (g) A reaction mixture initially contains a CO concentration of 0.1550 M and a Cl2 concentration of 0.171 M at 1000 K. What is the equilibrium concentration of CO at 1000 K. What is the equilibrium concentration of Cl2 at 1000 K? What is the equilibrium concentration of COCl2 at 1000 K? Express all answers to three significant figures

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Expert Solution

                                CO (g)     +        Cl2 (g)      ⇌ COCl2 (g)       Kc = 255

Initial                      0.1555                0.171                  0

at equilibrium            0.1555 -x         0.171-x                 x

      Kc = [COCl2]/ [CO] [Cl2]

      255 = x / (0.1555-x) (0.171-x)

   255 x2 - 84.2575 x + 6.78 = 0

   On solving,   x = 0.1386 M

Therefore, equilibrium concentrations are

   [CO] = 0.1555 -x = 0.1555 -0.1386 = 0.0169 M

    [Cl2] = 0.171 - x = 0.171 - 0.1386 = 0.0324 M

[COCl2] = 0.1386 M

queen_honey_blossom answered 2 years ago
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