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At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g)...

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g) + 2B(g) <===> 4C(g) K(c) = 2.93 x 10^(27) If, at this temperature, 2.40 mol of A and 3.70 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium? [A] = ? M [B] = ? M [C] = ? M

Solutions

Expert Solution

3A(g) + 2B(g) <===> 4C(g)

K(c) = 2.93 x 10^(27)

               3A(g) + 2B(g) <===> 4C(g)

I             2.4         3.7                 0

C          -3x       -2x                  4x

E         2.4-3x    3.7-2x                4x

         Kc   = [C]^4/[A]^3[B]^2

      2.93*10^27   = (4x)^4/(2.4-3x)^3*(3.7-2x)^2

   2.93*10^27*(2.4-3x)^3*(3.7-2x)^2   = 256x^4

            x   = 0.79

[A]   = 2.4-3x = 2.4-3*0.79   = 0.03M

[B]    = 3.7-2x   = 3.7-2*0.79    = 2.12M

[C]   = 4x          = 4*0.79          = 3.16M

queen_honey_blossom answered 2 years ago
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