Chemical Reaction Kinetics and Factors Affecting Reaction Rates Quiz

Temperature affects reaction rates by altering molecular speeds and collision frequency.

Higher reactant concentration leads to more frequent collisions, thus accelerating the reaction.

Catalysts lower activation energy, enabling the reaction to proceed faster without being used up.

Raising temperature boosts molecular speed and collision frequency, thus accelerating reactions.

Second-order reactions exhibit a direct relationship between reactant concentration and reaction rate.

Volume typically does not influence reaction rates, as they're determined by concentrations.

Order defines the relationship between reactant concentration and reaction rate.

Activation energy is the energy barrier that reactants must overcome for a reaction to occur.

Surface area affects reaction rates by altering the frequency of collisions between reactant molecules.

In zero-order reactions, the rate remains constant regardless of reactant concentration changes.

Arrhenius equation links reaction rate constants with temperature, showing how temperature affects reaction rates.

Zero-order kinetics exhibit constant reaction rates and half-lives irrespective of reactant concentrations.

Half-life remains constant regardless of the initial concentration in first-order reactions.

Enzymes facilitate reactions by lowering the activation energy, hence speeding up the process.

Doubling the concentration of one reactant in a second-order reaction doubles the reaction rate.

The rate-determining step dictates the overall speed of a reaction as it is the slowest step.

Transition state represents the highest energy point in a reaction, separating reactants from products.

Reaction mechanism details the individual steps through which reactants transform into products.