Explanation:

In a chemical reaction, the rate constant (k) is a proportionality constant that relates the rate of the reaction to the concentration of the reactants. The units of the rate constant depend on the order of the reaction.

Zero-Order Reaction:
In a zero-order reaction, the rate of the reaction is independent of the concentration of the reactants. It means that the rate of the reaction is constant over time. The rate equation for a zero-order reaction is given by:

rate = k

The units of the rate constant (k) for a zero-order reaction can be determined by considering the units of the rate. The rate of a reaction is typically expressed in terms of concentration per unit time (mol L^-1 s^-1). Therefore, the units of the rate constant for a zero-order reaction would be:

[k] = (mol L^-1 s^-1)

Second-Order Reaction:
In a second-order reaction, the rate of the reaction is proportional to the square of the concentration of one reactant or the product of the concentrations of two reactants. The rate equation for a second-order reaction is given by:

rate = k[A]^2 or rate = k[A][B]

The units of the rate constant (k) for a second-order reaction can be determined by considering the units of the rate and the concentrations. Since the rate is typically expressed in terms of concentration per unit time (mol L^-1 s^-1), the units of the rate constant would be:

[k] = (mol L^-1 s^-1)/(mol^2 L^-2) = (L mol^-1 s^-1)

Difference in Units:
From the above explanations, it is clear that the units of the rate constant for a zero-order reaction are different from the units of the rate constant for a second-order reaction. Therefore, the statement is false. The unit of the rate constant for a zero-order reaction is different from the unit of the rate constant for a second-order reaction.