zeroorderkinetik

Zero-order kinetics is a type of reaction rate that is independent of the concentration of the reactants. In this type of kinetics, the rate of the reaction remains constant throughout the process, regardless of how much reactant is left. This is in contrast to first-order and second-order kinetics, where the rate of the reaction depends on the concentration of the reactants.

Zero-order reactions are often observed in reactions where the rate-determining step involves a surface reaction, such as in heterogeneous catalysis or in reactions involving solids. In these cases, the rate of the reaction is determined by the availability of active sites on the surface of the solid, rather than the concentration of the reactants in solution.

The rate law for a zero-order reaction can be expressed as:

Rate = k

where k is the rate constant. The integrated rate law for a zero-order reaction is:

[Reactant] = -kt + [Reactant]0

where [Reactant]0 is the initial concentration of the reactant. This equation shows that the concentration of the reactant decreases linearly with time, which is a characteristic feature of zero-order reactions.

Zero-order kinetics can also be observed in reactions where the reactants are continuously replenished, such as in biological systems where enzymes are constantly produced. In these cases, the rate of the reaction remains constant because the concentration of the reactants is maintained at a constant level.