Interpretation:
The correct statement about the reaction process at equilibrium needs to be determined.
Concept introduction:
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.
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.
Chapter U6 Solutions
Living by Chemistry
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