Which factor does NOT increase the rate of a chemical reaction by increasing the number of effective collisions between reactant molecules?

A. Increasing the temperature

B. Increasing the concentration of reactants

C. Decreasing the surface area of solid reactants

D. Adding a catalyst

What is the primary reason for an increase in the rate of reaction when the temperature is raised?

A. More reactant molecules are present

B. Reactant molecules move slower

C. Reactant molecules have higher kinetic energy

D. Activation energy of the reaction decreases

Which statement about catalysts is FALSE?

A. Catalysts lower the activation energy of a reaction

B. Catalysts are consumed in the reaction

C. Catalysts increase the rate of reaction

D. Catalysts do not change the equilibrium position of a reaction

For a first-order reaction, if the concentration of the reactant is halved, the half-life will:

A. Remain the same

B. Double

C. Halve

D. Quadruple

The units of the rate constant for a zero-order reaction are:

A. s^-1

B. M^-1 s^-1

C. M s^-1

D. No units

a) Explain the concept of activation energy in the context of collision theory. [3]

b) How does an increase in temperature affect the rate of a reaction according to collision theory? [2]

a) Describe the effect of a catalyst on the activation energy of a reaction. [2]

b) Using collision theory, explain why increasing the concentration of reactants generally increases the rate of a reaction. [3]

a) What is meant by the term "order of reaction"? [2]

b) If a reaction has a half-life that remains constant regardless of the initial concentration of the reactant, what can be deduced about the order of the reaction? [3]

a) Define the term "rate constant" in the context of reaction kinetics. [2]

b) How does the rate constant vary with temperature for a typical chemical reaction? [2]

c) Using collision theory, explain the effect of increasing the surface area of a solid reactant on the rate of a reaction. [3]

a) Describe the role of a catalyst in terms of its effect on the energy profile of a reaction. [3]

b) What is meant by the standard enthalpy change of formation? [2]

c) How can Hess's Law be used to determine the enthalpy change of a reaction? [3]