Question

Which statement about reversible reactions is correct? At equilibrium, the forward and reverse reactions stop at the appropriate concentrations. At equilibrium, the forward and reverse reactions continue indefinitely. At equilibrium the rate of reaction of products divided by the rate of reaction of reactants equal the equilibrium constant, K.

Answer 1

The correct answer is At equilibrium the rate of reaction of products divided by the rate of reaction of reactants equal the equilibrium constant, K.

The chemical reactions which occurs in forward direction as well as backward direction under particular conditions is said to be reversible reactions. In these reactions, concentration of reactants and products remain same and both reactions i.e. forward and backward reactions occurs at similar rates.

Equilibrium is the state of reaction in which formation of reactants into products and formation of products into reactants occurs simultaneously at similar rate.

Now, equilibrium constant is equal to the ratio of concentration of the products to the concentration of the reactants.

For example: $A+B\rightarrow C+D$

$k = \frac{[C][D]}{[A][B]}$

Since, rate of reaction is directly proportional to the equilibrium constant i.e.

$k_{eq}= \frac{rate of reaction of product}{rate of reaction of reactant}$

= $\frac{\frac{d[C][D]}{dt}}{\frac{d[A][B]}{dt}}$

Thus, equilibrium constant is equal to the ratio of rate of reaction of product to the rate of reaction of reactant at equilibrium.

Answer 2

Answer:

At equilibrium, the forward and reverse reactions continue indefinitely.

Explanation:

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