Question

consider the reaction x → y + z. which of the following is a possible rate law? a rate = k y b rate = k y z c rate = k x z d rate = k x question 3

Explanation:

Step1: Recall rate - law concept

The rate - law of a reaction is expressed in terms of the concentration of the reactants. For a reaction \(X
ightarrow Y + Z\), the rate of the reaction depends on the concentration of the reactant \(X\). The rate constant \(k\) is a proportionality constant.

Step2: Analyze each option

• Option A: rate \(=k[Y]\) is incorrect because the rate of the forward reaction \(X

ightarrow Y + Z\) should not depend on the concentration of the product \(Y\) in a simple one - step reaction.

• Option B: rate \(=k[Y][Z]\) is incorrect as it depends on the concentrations of the products \(Y\) and \(Z\), not the reactant.
• Option C: rate \(=k[X][Z]\) is incorrect since \(Z\) is a product and the rate of the forward reaction is not based on the concentration of a product in a simple reaction.
• Option D: rate \(=k[X]\) is correct as the rate of a simple one - step reaction \(X

ightarrow Y + Z\) is proportional to the concentration of the reactant \(X\).

Answer:

D. rate \(=k[X]\)