Question

Consider the following multistep reaction: A+B→AB(slow) A+AB→A2B(fast)−−−−−−−−−−−−−−−−− 2A+B→A2B(overall) Based on this mechanism, determine the rate law for the overall reaction.

Answer 1

Answer:

r = k × [A] × [B]

Explanation:

To determine the rate law, we simply use the slow step reaction equation. The slow step is the rate determining step in the reaction.

A+B→AB

And as we know, the rate of the reaction is proportional directly to the product of the concentration of the reactants which concentration is changing over the course of the reaction.

r = k × [A] × [B]

Where r = rate of reaction

k = reaction rate constant

[A] = Concentration of molecule A

[B] = Concentration of molecule B

Answer 2

The rate law for the overall reactions is $\rm r = k \times [A] \times [B]$

What is the rate law?

The rate law of the reaction shows how the reaction depends on reactant concentration.

In a mathematical equation, a rate law connects the concentration of a reactant to the reaction rate.

It's represented as rate = k[reactant1][reactant2], with k being a reaction-specific rate constant.

$\rm r = k \times [A] \times [B]$

Where r = rate of reaction

[A] = Concentration of molecule A

[B] = Concentration of molecule B

Thus, the rate law for the reaction is  $\rm r = k \times [A] \times [B]$

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