Question

At equilibrium, the rate of forward reaction is equal to the rate of backward reaction.
(A) True
(B) False

Answer 1

We know that an equilibrium is a condition in which properties like temperature, pressure and concentration of the system does not show any change with the passage of time. The mixture of reactants and products in the equilibrium state is known as the equilibrium mixture. There are two types of equilibrium: - physical equilibrium and chemical equilibrium.

Complete step-by-step answer: Here we will talk about chemical equilibrium.
Chemical equilibrium is the state of a chemical reaction in which the rate of forward reaction is equal to the rate of backward reaction. The result of this equilibrium will be that the concentration of the reactants and products will remain constant.
But this does not mean that the chemical reaction has ceased. Chemical equilibrium is in a dynamic state in which the reactants are being converted into the products and the products are being converted back into reactants at all time.
The relationship between forward and reverse reactions in a dynamic equilibrium can be expressed as:
$aA + bB \rightleftharpoons mC + nD$
${K_{eq}} = \dfrac{{{{[C]}^m}{{[D]}^n}}}{{{{[A]}^a}{{[B]}^b}}}$
Here ${K_{eq}}$ is known as the equilibrium constant.
This relationship comes under the law of mass action which states that the rate of a chemical reaction at a given temperature is directly proportional to the product of active masses of the reactants.

So, the correct answer will be Option A i.e. True.

Note: A catalyst usually speeds up a chemical reaction but it will have no effect on the equilibrium position of that reaction. Always remember this that while writing the equilibrium constant expression, the concentration of the products will go in the numerator and the concentration of the reactants will go in the denominator.