The equilibrium will shift to the right, favoring the formation of more product.
So, in order to determine whether or not a reaction is at equilibrium, you must calculate the reaction quotient, or Qc.
Qc expressed the ratio of products to reactants at a given instant. If the value you obtain for Qc is smaller than Keq, the equilibrium constant, there are more reactants than products, which will cause the equilibrium to shift to the right, favoring the formation of more products.
If Qc is bigger than Keq, there are more products than reactants, which will cause the equilibrium to shift ot the left, favoring the formation of more reactants.
If Qc is equal to Keq, the reaction is at equilibrium and no shift will take place.
Qc=[B][A]=0.100 mol/L0.020 mol/L=5.0
Notice that Qc is smaller than Keq, which is said to be 10.0. This means that the reaction will shift to the right and favor the formation of more product.
