Understanding the Rate Law

The rate law tells us how the rate of a reaction changes with the concentration of the reactants. It's typically written in the form:

* Rate = k[A]^m[B]^n

Where:

* Rate is the speed of the reaction.

* k is the rate constant (a specific value for the reaction).

* [A] and [B] are the concentrations of reactants A and B.

* m and n are the orders of the reaction with respect to A and B, respectively. These exponents determine how the concentration of each reactant affects the rate.

The Specific Rate Law in Question

You've provided a rate law: kNO2H2. Let's assume this means:

* Rate = k[NO]^2[H2]

The Effect of Doubling [NO]

In this rate law, the concentration of NO is raised to the power of 2. This means the reaction is second order with respect to NO. Here's how the rate changes:

* If you double [NO], the rate will increase by a factor of 2^2 = 4.

In summary:

Doubling the concentration of NO in a reaction with the rate law kNO2H2 will quadruple (increase by a factor of 4) the rate of the reaction.