One example of a zero-order reaction is the decomposition of ammonia on a hot platinum wire, \(2 \mathrm{NH}_{3}(\mathrm{g}) \longrightarrow \mathrm{N}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) .\) If the concentration of ammonia is doubled, the rate of the reaction will (a) be zero; (b) double; (c) remain the same; (d) exponentially increase.

Chemical kinetics is the area of chemistry that concerns the rates at which chemical reactions occur. It dives into understanding how various factors, like temperature, pressure, and concentration of reactants, affect the speed of a reaction. It also involves the study of reaction mechanisms and the pathway by which a reaction proceeds.

Zero-order reactions fall under the canopy of chemical kinetics, where the rate is independent of the concentration of the reactants. This peculiarity makes zero-order reactions especially interesting because no matter how much you increase or decrease the concentration, the reaction pace stays unwavering. This equilibrium is sustained until one of the reactants is completely consumed, at which point the reaction stops abruptly. Zero-order kinetics are often found in processes that are catalyzed by enzymes or on surfaces where the catalyst is saturated.

The reaction rate, simply put, is how swiftly a reaction proceeds. It is typically measured by the change in concentration of reactants or products per unit time. In formulas, it can be represented as the negative of the change in concentration of reactants divided by the change in time (for a disappearance) or the positive of the change in concentration of products divided by the change in time (for an appearance).

In a zero-order reaction, where the reaction rate is measured as Rate = k[A]^0, the superscript '0' notates that the rate of the reaction is not dependent on the concentration of reactant A. In this case, k is a constant known as the rate constant, which is specific to each chemical reaction at a given temperature. The reaction remains at a fixed pace because of a surface process or a catalyst that operates at full capacity and is not affected by how much reactant is present.

In most chemical reactions, the concentration of reactants is vital in determining the rate at which the reaction proceeds. Altering these concentrations typically speeds up or slows down the reaction accordingly. This relationship is often expressed in the rate law, which indicates how the rate is affected by the concentration of the reactants.

However, this is not the case with zero-order reactions. For these reactions, the rate law shows that the concentration of reactants plays no role in the speed of the reaction. The rate of a zero-order reaction is constant and given by the rate constant, which is not altered by changes in concentration. This exceptional attribute of zero-order kinetics is crucial for students to understand, as it deviates from the more common concentration-dependent reactions they might encounter.