Consider the reaction
Select a possible mechanism for the reaction.
Step1:2X2Y+Z2→2X2YZ (slow)
To determine a possible mechanism for the given reaction, we need to consider the stoichiometry of the reactants and products, as well as the rate-determining step.
The reaction equation is:
Step 1: 2X2Y + Z2 → 2X2YZ (slow)
Based on this equation, we can propose a possible mechanism involving two elementary steps:
Step 1: Formation of an intermediate
2X2Y + Z2 → X2Y-Z2 (fast)
Step 2: Rearrangement and regeneration of the product
X2Y-Z2 → 2X2YZ (fast)
In this mechanism, Step 1 involves the formation of an intermediate, X2Y-Z2, which is rapidly formed from the reaction of 2X2Y and Z2. This step is assumed to be fast as it does not appear in the rate equation.
Step 2 is the rearrangement of the intermediate, leading to the formation of the final product, 2X2YZ. This step is also assumed to be fast.
The slow step in the mechanism is Step 1, as it determines the overall rate of the reaction. The rate equation for this reaction would only involve the concentration terms for the reactants involved in Step 1.
It's important to note that this is just one possible mechanism for the given reaction. Other mechanisms may exist depending on the experimental conditions and other factors. Mechanisms are proposed based on experimental evidence and theoretical considerations, and further investigation may be required to validate a proposed mechanism.