AP Chemistry Unit 5 Kinetics

How is the rate constant (k) related to the slope of a concentration vs. time graph for a first order reaction?

• The slope of the [A] vs. time graph is equal to k.

• The slope of the ln[A] vs. time graph is equal to -k.

• The slope of the [A] vs. time graph is equal to -k.

• The slope of the ln[A] vs. time graph is equal to k.

What does the term 'activated complex' refer to?

• A stable arrangement of atoms in a chemical reaction.

• A temporary, unstable arrangement of atoms during the transformation of reactants into products.

• A type of catalyst that speeds up reactions.

• The final product of a chemical reaction.

What is the rate law for a reaction?

• Rate = k[A]^n[B]^m, where k is the rate constant, and n and m are the orders of the reaction with respect to reactants A and B.

• Rate = k[A] + k[B], where k is the rate constant for a first-order reaction.

• Rate = k[A]^2 + k[B]^2, indicating a second-order reaction with respect to both reactants.

• Rate = k[A]/[B], representing an inverse relationship between the reactants.

How are the orders of a reaction determined experimentally?

• Through theoretical calculations based on stoichiometry.

• By measuring the change in concentration over time using the method of initial rates or integrated rate laws.

• By observing the color change of the reactants.

• By using a catalyst to speed up the reaction and measuring the time taken.

What does a first order reaction mean?

• A first order reaction is one where the rate of reaction is directly proportional to the concentration of one reactant. The rate law can be expressed as Rate = k[A], where k is the rate constant.

• A first order reaction is one where the rate of reaction is independent of the concentration of reactants.

• A first order reaction involves two reactants and the rate is proportional to the product of their concentrations.

• A first order reaction has a constant rate regardless of the concentration of reactants.

What is a reaction intermediate?

• A species that is formed in one step of a reaction mechanism and consumed in a subsequent step.

• A catalyst that speeds up a chemical reaction without being consumed.

• A final product of a chemical reaction that is stable and does not change.

• A reactant that is present in the overall balanced equation.

What is the significance of the slope in a concentration vs. time graph for a second order reaction?

• The slope indicates the rate constant k, which is equal to the concentration of the reactant.

• The slope is constant and does not change with time.

• The slope of the 1/[A] vs. time graph is equal to k, indicating that the rate depends on the square of the concentration of the reactant.

• The slope represents the first derivative of concentration with respect to time.

What is the integrated rate law for a first order reaction?

• ln[A] = -kt + ln[A]₀, where [A]₀ is the initial concentration.

• 1/[A] = kt + 1/[A]₀, where [A]₀ is the initial concentration.

• [A] = [A]₀ e^(-kt), where [A]₀ is the initial concentration.

• ln[A] = kt + ln[A]₀, where [A]₀ is the initial concentration.

What is the difference between a catalyst and a reaction intermediate?

• A catalyst is a substance that increases the rate of a reaction without being consumed, while a reaction intermediate is formed and consumed during the reaction.

• A catalyst is a substance that slows down a reaction, while a reaction intermediate is a final product of the reaction.

• A catalyst is a product of the reaction, while a reaction intermediate is a reactant that is not consumed.

• A catalyst is a substance that changes the color of the reactants, while a reaction intermediate is a gas released during the reaction.

What is the Arrhenius equation?

• k = Ae^(-Ea/RT), where A is the pre-exponential factor.

• k = A + Ea/RT, where A is the activation energy.

• k = A * T^Ea, where A is the rate constant.

• k = A - Ea/RT, where A is the temperature.