AP Chemistry kinetics rate laws key terms

What is a rate law?

An equation that relates the reaction rate to the concentration of reactants, often in the form: Rate = k[A]^m[B]^n.

Define reaction order.

The sum of the exponents in a rate law, indicating how the rate depends on concentrations of reactants.

True or false: Rate constants vary with temperature.

True, because the rate constant (k) changes as temperature affects the energy and frequency of collisions.

What does the symbol 'k' represent?

'k' is the rate constant, specific to each reaction at a given temperature, affecting the reaction rate.

Fill in the blank: For a first-order reaction, Rate = _____.

Rate = k[A], where [A] is the concentration of the reactant.

Difference between zero-order and first-order reactions?

Zero-order: Rate is constant, independent of concentration. First-order: Rate depends linearly on concentration.

What is the half-life of a reaction?

The time required for the concentration of a reactant to reduce to half of its initial value.

Define activation energy (Ea).

The minimum energy needed for a chemical reaction to occur, represented in the Arrhenius equation.

True or false: Catalysts affect the rate constant.

False, because catalysts lower activation energy without changing the rate constant itself.

What is a differential rate law?

An expression that shows how the rate depends on the concentration of reactants, typically in the form of a function.

How does temperature affect reaction rates?

Increasing temperature generally increases reaction rates by increasing the kinetic energy of molecules.

What is a complex reaction?

A reaction that involves multiple elementary steps, each with its own rate law.

Define integrated rate law.

An equation that relates concentration and time, used to calculate concentrations at different times.

True or false: Rate laws must be determined experimentally.

True, because the form and constants of rate laws cannot be deduced from stoichiometry alone.

What is the Arrhenius equation?

$\displaystyle k = Ae^{-\\frac{E_a}{RT}}$, where A is the pre-exponential factor, Ea is activation energy, R is the gas constant.