Consider the reaction and its rate law.

2A+3B⟶products
rate=k[B]2
What is the order with respect to A?
What is the order with respect to B?
What is the overall reaction order?

The order of the reaction with respect to A is 0.

The order of the reaction with respect to B is 2.

Overall reaction order for the given reaction 2.

From the question,

The rate law for the given reaction is  

Rate = k[B]²

This means the rate of the reaction is solely dependent on the concentration of B.

The rate law for the reaction can also be written as

Rate = k[B]²[A]⁰

From the rate law above, we can deduce that

The order of the reaction with respect to A is 0. That is, zero order

Also,

The order of the reaction with respect to B is 2. That is, second order.

Now, for the overall reaction order

Overall reaction order is the sum of the powers to which all reactant concentrations appearing in the rate law are raised.

∴ Overall reaction order for the given reaction = 2 + 0 = 2. That is, the reaction is second order reaction overall

Hence,

The order of the reaction with respect to A is 0.

The order of the reaction with respect to B is 2.

Overall reaction order for the given reaction 2.

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The order with respect to A is 2

The order with respect to B is 0.

The overall reaction order is 2.

Explanation:

The rate of chemical equation is represented by its rate equation. Here the rate equation of the given chemical reaction is

Here k represents the rate constant .

Order of the reaction with respect to its individual reactants is represented by the power of the the reactants in the rate equation.

Here the power of the reactant A is 0 and the power of reactant B is 2.

Hence the order with respect to A is 0 and order with respect to B is 2.

The overall order of the reaction is given by the sum of the powers of the reactants in the rate equation.

Hence the total order=2+0=2

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