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]

Which factor does NOT affect the activation energy of a reaction?

A. Temperature

B. Catalyst

C. Concentration

D. Surface area

In the context of collision theory, which statement is TRUE?

A. All collisions lead to a reaction

B. Only collisions with energy greater than the activation energy lead to a reaction

C. Collisions with energy less than the activation energy lead to a reaction

D. The orientation of colliding particles does not matter

How does increasing the surface area of a solid reactant affect the rate of reaction?

A. It decreases the rate of reaction

B. It does not affect the rate of reaction

C. It increases the rate of reaction

D. It makes the reaction reach equilibrium faster

For a reaction to be second order with respect to a particular reactant, the rate of reaction will:

A. Remain unchanged if the concentration of the reactant is doubled

B. Double if the concentration of the reactant is doubled

C. Quadruple if the concentration of the reactant is doubled

D. Halve if the concentration of the reactant is doubled

What is the effect of adding a catalyst to a reaction at equilibrium?

A. It shifts the equilibrium to the right

B. It shifts the equilibrium to the left

C. It does not affect the position of the equilibrium

D. It increases the activation energy of the reaction

a) Explain the significance of the activation energy in determining the rate of a reaction. [3]

b) How does the concentration of reactants influence the rate of a reaction? [2]

c) Describe the relationship between the half-life and the order of a reaction. [3]

a) What factors can affect the activation energy of a reaction? [3]

b) Describe the effect of a catalyst on the rate of a reaction using collision theory. [3]

c) How can the order of a reaction be experimentally determined? [2]

a) Define the term "half-life" in relation to first-order reactions. [2]

b) How does the half-life of a first-order reaction compare to that of a zero-order reaction as the reaction progresses? [3]

c) Using collision theory, explain why an increase in temperature generally leads to an increase in the rate of a reaction. [3]

d) Describe the relationship between the rate constant, temperature, and the activation energy of a reaction. [4]

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

b) Describe how the concentration of a reactant affects the rate of a zero-order reaction. [3]

c) Explain the role of a catalyst in terms of its effect on the activation energy and the rate of a reaction. [3]

d) Using collision theory, describe the effect of increasing the concentration of reactants on the rate of a reaction. [4]

a) What is the significance of the activation energy in a chemical reaction? [3]

b) How does the presence of a catalyst affect the mechanism of a reaction? [3]

c) Describe the relationship between the rate of reaction and the frequency of effective collisions. [3]

d) Explain how the surface area of a solid reactant can influence the rate of a reaction. [3]