Answer:
The Keq (equilibrium constant) for a reaction is a measure of the extent to which the reactants are converted into products at equilibrium. It is determined by the concentrations of the reactants and products at equilibrium.
Step-by-step explanation:
Given that the Keq for the reaction A + B ⇌ AB is 6, we can interpret this as follows: at equilibrium, the concentration of AB is 6 times greater than the product of the concentrations of A and B. Now, let's consider the reaction 3 AB ⇌ 3 A + B. To find the Keq for this reaction, we need to compare the concentrations of the reactants and products at equilibrium. Since the stoichiometric coefficients of the reactants and products are all multiplied by 3 in the second reaction, we can say that the Keq for the second reaction will be the Keq for the first reaction raised to the power of 3. Therefore, the Keq for the reaction 3 AB ⇌ 3 A + B will be (6)^3 = 216. In summary, the Keq for the reaction 3 AB ⇌ 3 A + B is 216.