General Chemistry 004 - Test 2 Practice Flashcards

These flashcards cover key concepts from the General Chemistry lecture notes about kinetics, reaction rates, and equilibrium.

carbon-11

An isotope used in biomedical imaging with a half-life of 20.39 minutes.

half-life

The time required for half of a given sample to decay.

rate law

An equation that relates the rate of a reaction to the concentrations of reactants.

reaction rate

The speed at which reactants are converted into products.

zero order reaction

A reaction whose rate is constant and independent of the concentration of reactants.

first order reaction

A reaction where the reaction rate is directly proportional to one reactant's concentration.

second order reaction

A reaction whose rate depends on the square of the concentration of one reactant or the product of the concentrations of two reactants.

activation energy

The minimum energy required to initiate a chemical reaction.

catalyst

A substance that increases the rate of a reaction without being consumed.

equilibrium constant (K)

A number that expresses the ratio of the concentrations of products to reactants at equilibrium.

Le Chatelier's principle

A principle stating that if a stress is applied to a system at equilibrium, the system adjusts in a way that counteracts the stress.

intermediate

A species formed during the reaction that is not included in the overall reaction.

homogeneous catalyst

A catalyst that is in the same phase as the reactants.

heterogeneous catalyst

A catalyst that is in a different phase than the reactants.

average reaction rate

The change in concentration of reactants or products over a specified period.

reaction quotient (Q)

A measure of the relative amounts of products and reactants present in a reaction at any given time.

dynamic equilibrium

A state of balance where the rates of the forward and reverse reactions are equal.

molecularity

The number of molecules involved in a reaction step.

rate-determining step

The slowest step in a reaction mechanism that controls the overall reaction rate.

frequency factor (A)

A constant that represents the frequency of collisions in the context of the Arrhenius equation.

pressurized equilibrium

A state of balance that occurs when gas reactants and products are contained at high pressure.