If the equilibrium constant for this reaction is Kc = 248, predict, if possible,
ID: 828356 • Letter: I
Question
If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will
happen when the reactants and product are combined with the concentrations shown.
[CO] = [Cl2] = 0.010 M; [COCl2] = 0.070 M
A) The reaction will proceed to the right.
B) The reaction will proceed to the left.
C) The reaction is at equilibrium, and no change in concentrations will occur.
D) The container volume needs to be specified before a prediction can be made.
E) The temperature needs to be specified before a prediction can be made.
Please explain or show work.
Explanation / Answer
Well we know that is Q (reaction quotient) is larger than K that means the reaction will shift to the right or products. Before I tell you the answer, I'll explain a very easy way on how to know if the reaction will shift left or right.
Lets say hypothetically Q=1 and K= 1/2
-Now we know that the equation for both is ALWAYS Products/ reactants. So if K has more reactants than products ( from the 1/2 remember products over reactants) than the formula will shift to the right to create more products to reach equilibrium.
Now lets do your problem
.0100M / .07x 2 ( no exponents since they are all one moles of the gas). This equals .101
Now .071 is WAY less than K( which is 248) so the reaction will shift to the reactants or the left.