Question

The equilibrium constant for the gaseous reaction:

C + D ⇌ E + 2F

is 3.0 at 50 °C. In a 2.0 L flask at 50 °C are placed 1.0 mol of C, 1.0 mol of D, 1.0 mol of E, and 2.0 mol of F.

a) Is the system at equilibrium? Explain how you know.

b) If the system is not in equilibrium, in which direction will the reaction proceed more rapidly until equilibrium is reached?

Answer 1

C     +      D   <------------->   E   +   2 F

1.0        1.0                        1.0      2.0

Q = [E][F]^2 / [C][D]

   = (1.0)(2.0)^2 / (1 x 1)

Q = 4.0

K = 3.0

equilibrium constant and reaction quotient are not equal.

K < Q .

so the reaction shifts back ward direction , that means reactants favoured . reaction shifts to left side to reach equilibrium