A mixture initially contains AA, BB, and CC in the following concentrations: [A][A]A_1 = 0.550 MM, [B][B]B_1 = 1.40 MM, and [C][C]C_1 = 0.600 MM. The following reaction occurs and equilibrium is established: A+2B⇌CA+2B⇌C At equilibrium, [A][A]A_2 = 0.430 MM and [C][C]C_2 = 0.720 MM. Calculate the value of the equilibrium constant, KcKcK_c.

The value of the equilibrium constant KC is 1.244

Explanation:

A mixture initially contains A, B, and C in the following concentrations: [A] = 0.550 M, [B] = 1.40 M, and [C] = 0.600 M. The following reaction occurs and equilibrium is established: A+2BC

At equilibrium, [A] = 0.430 M and [C] = 0.720 M. Calculate the value of the equilibrium constant, Kc

Step 1: The balanced equation

A+2BC

Step 2: The initial concentrations

[A] = 0.550 M

[B] = 1.40 M

[C] = 0.600 M

Step 3: The concentraions at equilibrium

[A] = 0.550 - X = 0.430 M

[B] = 1.40 - 2X M

[C] = 0.600 + X = 0.720 M

X = 0.120 M

[A] = 0.550 - 0.120 = 0.430 M

[B] = 1.40 - 2*0.120 = 1.16 M

[C] = 0.600 + 0.120 = 0.720 M

Step 4: Calculate Kc

Kc = [C] / [A][B]²

Kc = 0.720 / (0.430*1.16²)

Kc = 1.244

The value of the equilibrium constant KC is 1.244