For a zero-order reaction, what is the relationship between concentration and rate?

In a zero-order reaction, the rate of the reaction is independent of the concentration of the reactants. This means that regardless of how much of the reactant is present, the rate at which the reaction proceeds remains constant. The rate can be expressed by the rate law for a zero-order reaction, which is simply:

Rate = k

where k is the rate constant. This relationship shows that the rate does not change with varying concentrations of the reactants; hence, increasing or decreasing the concentration does not have any impact on the rate of the reaction.

In scenarios where concentrations are high, low, or remain unchanged, the reaction continues at the same rate set by the constant k. This is characteristic of zero-order kinetics, typically observed under conditions where a reactant is saturated, leading to constant rate behavior, often in reactions occurring on a surface or where a catalyst is involved.