1. Run multiple trials with different reactant concentrations. 2. Observe how the rate changes with each concentration change. 3. Use this data to determine the reaction orders and rate constant.

The study of reaction rates.

The speed at which reactants are converted into products, measured by tracking the change in concentration of reactants or products over time.

An equation that shows how the rate of a reaction depends on the concentrations of reactants; determined experimentally.

A proportionality constant specific to each reaction at a given temperature, indicating how fast a reaction proceeds.

The time it takes for the concentration of a reactant to decrease by half.

A single-step reaction where the rate law can be directly determined from its stoichiometry.

The minimum energy needed for a reaction to occur; the energy difference between reactants and the activated complex.

A series of elementary steps that describe how a reaction occurs.

A substance that speeds up a reaction without being consumed by providing an alternative pathway with lower activation energy.

Increasing temperature generally increases the rate constant (k), leading to a faster reaction.

A catalyst lowers the activation energy of a reaction.

The reaction rate doubles.

The reaction rate quadruples.