Question

A mixture is prepared with [CO] = 0.035, [Cl2] = 0.015, and [COCl2] = 0.95. It is known that Kc for the equilibrium is 1.2 x 10-3
at 400OC. Predict what will happen.

Choose one answer.

a. The reaction is at equilibrium so no net reaction occurs.

b. The reaction occurs in the forward direction.

c. The reaction occurs in the reverse direction.

d. It is impossible to predict without more information.

Answer 1

Write the equation.
Write the expression for Kc.
Substitute into Kc and calculate the reaction quotient, Q. Compare that with Kc.
If Q<Kc, it means the numerator is too small, the denominator is too large, and the reaction will go to the right.
If Q>Kc, it means the numerator is too large, the denominator is too small, and the reaction will go to the left.
If Q=Kc, the reaction is at equilibrium.

Answer 2

I CALCULATED IT OUT TO Q = 1.80*10^3
SO IT WAS A RIGHT SHIFT FORWARD BC Q<K meaning that substances on left react to form substances on the left to reach eq...


SO I GOT B as the answer
IS THAT CORRECT????

Answer 3

To calculate Q all you have to do is treat it like a K. Q = C(COCl2)/C(Cl2)*C(CO). This equals 1.8 x 10^3. We can see now that Kc < Q therefore the reaction will proceed to the left. If it were Kc > Q then it would proceed to the right.