Question

1) According to the collision theory of kinetics, which statement best describes the rate of a chemical reaction?

a. The greater the difference in energy between the reactants and products, the faster is the reaction

b. All collisions between molecules with at least a minimum kinetic energy result in reaction.

c. All collisions between molecules with at least a minimum kinetic energy and the proper orientation result in reaction.

d. The greater the difference in energy between the reactant and transition state, the faster is the reaction.

e. All collisions result in a chemical reaction.

2) Which of the following statements is FALSE?

a. The transition state is a short-lived, high energy state, intermediate between reactants and products.

b. A catalyst alters the rate of a reaction and is neither a product nor a reactant in the overall equation.

c. In order for a reaction to occur, reactant molecules must collide.

d. A reaction of the form, 2 A + B → products, will usually have a one-step mechanism.

e. The rate of the bimolecular reaction A + B → products is proportional to the frequency of collisions between A and B.

Answer 1

1) A:- C.All collisions between molecules with at least a minimum kinetic energy and the proper orientation result in reaction.

Explanation:-

For any chemical reaction the minimum amount of energy is needed i.e. activation energy for occur collision between reactant and the proper orientation is takes place.

2)

A:- d.False => d. A reaction of the form, 2 A + B → products, will usually have a one-step mechanism.

Explanation:

Actually the given reaction 2 A + B → products, not usually have a one-step mechanism. For that this statement is false statement.