Question

Consider the equilibrium reaction: 3CIO-(aq) ↔ CIO3-(aq) + 2CI-(aq)The equilibrium constant Kc = 3.2 X 103. The following concentrations are present: [Cl-] = 0.50 mol/L; [ClO3-] = 0.32 mol/L; [ClO-] = 0.24 mol/L. Is the mixture at equilibrium and, if not, in which direction will reaction proceed?​

Answer 1

Answer:

tthhhshbsbnsnnsnnenbsbbben

Answer 2

Answer: Right shift

Explanation:

We have to know the Reaction quotient Qc, and the formula for Qc is the same as Kc, but instead of measuring equilibrium, it's like a snapshot of the reaction showing where it is. Too many products? Make some more reactants. Too many reactants? Make more products. Or if the reaction is at equilibrium.

Q < Kc -> right shift

Q > Kc -> left shift

Q = Kc -> equilibrium

For this problem,

Qc = (0.5)^2*(0.32)/(0.24)^3 = 5.78

5.78 < 3.2*10^3

So we gotta make more product by right shifting the reaction.