Chemistry Rate Laws

Every equation that needs to be memorized for rate laws.

Zeroth Order Reaction Rate Law

A zeroth order reaction maintains a constant rate over time, unaffected by changes in reactant concentrations, until the reactants are fully consumed.

Zeroth Order Integrated Rate Law

For zeroth order reactions, the integrated rate law is expressed as [A] = [A]₀ - kt, where [A] is the concentration at time t, [A]₀ is the initial concentration, k is the rate constant, and t represents time.

Zeroth Order Half-Life Equation

The half-life (t₁/₂) for a zeroth order reaction is calculated using t₁/₂ = [A]₀ / (2k), indicating the duration it takes for the reactant concentration to reduce by half.

First Order Reaction Rate Law

In a first order reaction, the rate is directly proportional to the concentration of a single reactant. As the concentration of this reactant increases, the reaction rate also rises.

First Order Integrated Rate Law

The integrated rate law for a first order reaction is given as ln[A] = ln[A]₀ - kt, which can be rearranged to [A] = [A]₀ e^(-kt), demonstrating that the natural logarithm of concentration decreases linearly with time.

First Order Half-Life Equation

The half-life (t₁/₂) of a first order reaction is defined by t₁/₂ = 0.693 / k, signifying the time needed for the concentration to fall to half of its initial value.

Second Order Reaction Rate Law

In a second order reaction, the rate correlates to either the square of a single reactant's concentration or the product of the concentrations of two different reactants.

Arrhenius Equation

The Arrhenius equation describes the temperature dependence of reaction rates, expressed as k = Ae^(-Ea/(RT)), where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the universal gas constant, and T is the temperature in Kelvin.