Chapter U6, Problem 13STP

Interpretation Introduction

Interpretation:

The correct statement about the reaction process at equilibrium needs to be determined.

Concept introduction:

Chemical kinetic is the branch of chemistry that deals with kinetic or rate of a chemical reaction. The rate of reaction can be defined as the change in the concentration of reactant and product with time. The rate of reaction mainly depends on the activation energy.

For a chemical reaction to take place, the two important requirements are activation energy of the reactant molecules and the correct orientation of reactant molecules to collide to form product.

Answer to Problem 13STP

Option (A) is correct option.

Explanation of Solution

Reason for correct option:

In the rerversible reaction, reaction moves in both directions. The forward reaction converts the reactant molecule to product molecule and moves towards right. The backward reaction moves towards left side and converts products to reactant molecules.

When reaction reaches at equilibrium position, the rate of forward reaction is equal to rate of backward direction. In other words, the rate of consumption of reactant equals to rate of formation of product.

Conclusion

Reasons for incorrect options:

The equilibrium condition is not about mass or concentration of reactant and product. It is about rate of forward and backward reaction. Here rate of reaction indicates the change in the concentration of reactant and product with time.

Thus option (B), (C) and (D) are incorrect.