What is the rate of the following reaction (M/s) if the rate constant for the reaction is 0.500 L•mol-1•s-1 and the concentration of each reactant is 0.0628 M. (The units for the rate constant depend upon the rate law).

CO + NO2 --> CO2 + NO

The units tell you this is a second order reaction rate.An order of 1 for CO and 1 for NO2 would mean

rate = 0.500*(0.0628)(0.0628)

To determine the rate of the reaction, you need to use the rate law equation. The rate law equation gives the relationship between the rate of a reaction and the concentrations of the reactants.

The general form of the rate law equation is:
Rate = k[A]^m[B]^n

In this specific reaction, the rate law is unknown, so we need to determine it experimentally or analyze the mechanism of the reaction.

Given that the rate constant (k) for the reaction is 0.500 L•mol^(-1)•s^(-1) and the concentration of each reactant is 0.0628 M, we can assume a simplified rate law where the exponents (m and n) are both 1. This assumption is made for simplicity purposes.

Therefore, the rate law can be written as:
Rate = k[CO]^1[NO2]^1

Substituting the values:
Rate = (0.500 L•mol^(-1)•s^(-1))(0.0628 M)(0.0628 M)

After multiplying the values, the rate of the reaction would be given in the units of M/s.