Chemical Kinetics Overview

A substance that speeds up a chemical reaction without being consumed in the process.

The rate at which reactants are used up or products are formed in a chemical reaction.

The average rate of a reaction over a specific time interval. Calculated by dividing the change in concentration by the change in time.

The rate of a reaction at a specific point in time. Determined by finding the slope of the tangent line to the concentration versus time curve.

The instantaneous rate of a reaction at the beginning, when time is zero.

The decrease in the rate of a reaction as time progresses.

The maximum rate of a reaction, often observed at the beginning.

A reaction that has reached its final state, with no further changes in concentration.

A mathematical expression that describes the relationship between the rate of a reaction and the concentrations of the reactants. It provides a quantitative description of how the rate of a reaction changes as the concentrations of the reactants change.

The exponent of the concentration of a specific reactant in the rate law, which indicates how the rate of reaction changes as the concentration of that reactant changes.

A constant of proportionality in the rate law that reflects the intrinsic speed of a reaction under specific conditions (temperature, solvent).

A series of experiments designed to determine the rate law of a reaction by systematically varying the initial concentrations of reactants and observing the effect on the initial rate.

The sum of the individual reaction orders with respect to each reactant in the rate law; describes the overall sensitivity of the reaction rate to changes in reactant concentrations.

A reaction's rate changes based on factors like concentration, temperature, and catalyst presence.

The physical form of a reactant influences its rate. For example, a solid reactant in powder form will react faster than a solid tablet due to its larger surface area.

Increasing the concentration of reactants leads to a faster reaction rate because there are more molecules available to collide and react.

Higher temperatures increase the rate of a reaction because molecules move faster, collide more frequently, and with greater force.

A catalyst is a substance that speeds up a chemical reaction without being consumed in the process. Catalysts provide alternative reaction pathways with lower activation energies.

The minimum amount of energy that reacting molecules must possess to undergo a successful chemical reaction.

A higher temperature shifts the Boltzmann distribution curve to the right, increasing the fraction of molecules with enough energy to overcome the activation energy, thereby increasing the reaction rate.

The exponent of the concentration of a reactant in the rate law, which indicates how the rate of the reaction changes as the concentration of that reactant is changed. It's an integer that tells us how many molecules of that reactant are involved in the rate-determining step.

The overall order of a reaction is the sum of the individual orders of each reactant in the rate law.

The method of determining the rate law of a reaction by conducting a series of experiments in which the initial concentrations of the reactants are varied and the initial rate of the reaction is measured. We use the experimental data to deduce the orders of the reactants and the rate constant.

The step in a reaction mechanism that determines the overall rate of the reaction. It is the slowest step in the reaction mechanism.

A change in concentration over time. It can be expressed as the change in concentration of a reactant or product over a certain time interval.

A reaction mechanism is a series of elementary steps that describe the detailed pathway of a reaction. It shows the individual steps involved in the conversion of reactants to products.