Enter your **Initial Concentration [A₀]**, **Rate Constant (k)**, and **Time (t)** into the **Zero-Order Reaction Calculator** to find the **remaining concentration**, **Reaction Rate**, and **Percent Reacted** — just leave the field you want to solve for blank and hit **Calculate**.
Result
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Reaction Rate
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Percent Reacted
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A zero-order reaction is one where the reaction rate is independent of the concentration of the reactant. The rate remains constant throughout the reaction until the reactant is completely consumed.
For zero-order reactions, the rate constant k can be calculated using the integrated rate equation: [A] = [A₀] - kt. Rearranging gives k = ([A₀] - [A]) / t, where k has units of mol/L·s.
The half-life of a zero-order reaction is t₁/₂ = [A₀] / (2k). Unlike first-order reactions, the half-life depends on the initial concentration and increases as the reaction progresses.
In zero-order kinetics, the rate is constant and independent of concentration, while in first-order kinetics, the rate is proportional to the concentration. Zero-order reactions show linear concentration decrease over time.
Common examples include enzyme-catalyzed reactions at saturating substrate concentrations, surface-catalyzed reactions where the surface is fully occupied, and some photochemical reactions where light intensity is the limiting factor.
A zero-order reaction continues at a constant rate until one of the reactants is completely consumed. The time for complete consumption is t = [A₀] / k, after which the reaction stops abruptly.