Zero-Order Reaction Calculator

Calculate reaction rates, rate constants, and concentrations for zero-order kinetics reactions using integrated rate equations

mol/L

Initial concentration of reactant A

mol/L·s

Rate constant for zero-order reaction

s

Time elapsed since reaction start

Results

Result

--

Reaction Rate

--

Percent Reacted

--

Results Table

Frequently Asked Questions

What is a zero-order reaction?

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.

How do you calculate the rate constant for a zero-order reaction?

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.

What is the half-life of a zero-order reaction?

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.

How does zero-order kinetics differ from first-order kinetics?

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.

What are examples of zero-order reactions?

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.

When does a zero-order reaction end?

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.

More Chemistry Tools