Kinetics Quiz

What does the rate law for a reaction express?

• The dependence of the reaction rate on the concentration of products

• The dependence of the reaction rate on the concentration of reactants

• The change in concentration of reactants per unit time

• The change in concentration of products per unit time

Which of the following is NOT a factor that affects the rate of a chemical reaction?

• Temperature

• Catalyst

• Color of the reactants

• Concentration of reactants

• 1

• 2

• 3

• 4

What role does a catalyst play in a chemical reaction?

• It increases the concentration of reactants.

• It decreases the concentration of products.

• It provides an alternative pathway with a lower activation energy.

• It changes the equilibrium position of the reaction.

In the context of collision theory, what is required for a reaction to occur between two particles?

• They must collide with sufficient energy and proper orientation.

• They must be of opposite charges.

• They must collide with minimal energy but proper orientation.

• They must be in a liquid state.

What is the rate-determining step in a reaction mechanism?

• The fastest step in the sequence of steps leading to product formation

• The step that consumes the most energy

• The slowest step in the sequence of steps leading to product formation

• The step that produces the most product

For a first-order reaction, how does the rate change if the concentration of the reactant is doubled?

• The rate remains the same.

• The rate doubles.

• The rate quadruples.

• The rate is halved.

Which of the following statements about catalysts is FALSE?

• Catalysts are consumed in the reaction.

• Catalysts lower the activation energy of a reaction.

• Catalysts do not alter the equilibrium position of a reaction.

• Catalysts can be enzymes in biological systems.

What does the term "activation energy" refer to in a chemical reaction?

• The energy released when the reaction occurs

• The minimum energy required for reactants to transform into products

• The energy required to break bonds in the reactants

• The energy difference between the reactants and products

Which of the following is an example of a zero-order reaction?

• Decomposition of hydrogen peroxide in the presence of a catalyst

• The reaction between sodium thiosulfate and hydrochloric acid

• The Haber process for the synthesis of ammonia

• The decomposition of nitrogen dioxide at high temperatures