What are the factors that determine an effective collision?

Translational collision and energy of activation

Threshold energy and proper orientation

Proper orientation and steric bulk of the molecule

Collision frequency, threshold energy and proper orientation

In a chemical reaction, if the reactant requires a high amount of activation energy, then what is the behaviour of the reaction?

Doesn t depend on activation energy

Which of the following is a drawback of collision theory?

Have energy equal to or greater than the threshold energy

Which of the following explains the increase in the reaction rate by a catalyst?

Catalyst increases the number of collisions between the reacting molecules.

Catalyst decreases the rate of backward reaction so that rate of forward reaction increases

Catalyst provides extra energy to reacting molecules so that they produce effective collisions

Catalyst provides an alternative path of lower activation energy to the reactants

Catalyst increases the number of collisions between the reacting molecules.

Explore topic-wise MCQs in Chemistry.

This section includes 10 Mcqs, each offering curated multiple-choice questions to sharpen your Chemistry knowledge and support exam preparation. Choose a topic below to get started.

1.	What are the factors that determine an effective collision?
A.	Translational collision and energy of activation
B.	Threshold energy and proper orientation
C.	Proper orientation and steric bulk of the molecule
D.	Collision frequency, threshold energy and proper orientation
Answer» E.

Discussion

2.	In a chemical reaction, if the reactant requires a high amount of activation energy, then what is the behaviour of the reaction?
A.	Fast
B.	Slow
C.	Instantaneous
D.	Doesn t depend on activation energy
Answer» C. Instantaneous

Discussion

3.	What is the rate of reaction for a bimolecular elementary reaction?
A.	Z<sub>AB</sub> e<sup>-E<sub>a</sub>/RT</sup>
B.	Z<sub>AB</sub> e<sup>E<sub>a</sub>/RT</sup>
C.	Z<sub>AB</sub> e<sup>-E<sub>a</sub>/RT</sup>
D.	Z<sub>AB</sub> e<sup>E<sub>a</sub>/RT</sup>
Answer» B. Z<sub>AB</sub> e<sup>E<sub>a</sub>/RT</sup>

Discussion

4.	What is the term used to refer to the number of collisions per unit volume of the reaction mixture?
A.	Collision force
B.	Collision frequency
C.	Collision energy
D.	Collision time period
Answer» C. Collision energy

Discussion

5.	Which of the following is a drawback of collision theory?
A.	Proper orientation
B.	High activation energy
C.	Hard spheres
D.	Have energy equal to or greater than the threshold energy
Answer» D. Have energy equal to or greater than the threshold energy

Discussion

6.	The proper orientation of reactant molecules leads to bond formation.
A.	True
B.	False
Answer» B. False

Discussion

7.	Who put forward the collision theory of chemical reactions?
A.	Trautz and Lewis
B.	Luigi Galvani
C.	Henry Cavendish
D.	Alessandro Volta
Answer» B. Luigi Galvani

Discussion

8.	Effective collisions are those in which molecules must acquire the energy of activation.
A.	True
B.	False
Answer» B. False

Discussion

9.	Which of the following explains the increase in the reaction rate by a catalyst?
A.	Catalyst decreases the rate of backward reaction so that rate of forward reaction increases
B.	Catalyst provides extra energy to reacting molecules so that they produce effective collisions
C.	Catalyst provides an alternative path of lower activation energy to the reactants
D.	Catalyst increases the number of collisions between the reacting molecules.
Answer» D. Catalyst increases the number of collisions between the reacting molecules.

Discussion

10.	When a catalyst is involved in the collision between the reactant molecules, more energy is required.
A.	True
B.	False
Answer» C.

Discussion

Explore topic-wise MCQs in Chemistry.

What are the factors that determine an effective collision?

In a chemical reaction, if the reactant requires a high amount of activation energy, then what is the behaviour of the reaction?

What is the rate of reaction for a bimolecular elementary reaction?

What is the term used to refer to the number of collisions per unit volume of the reaction mixture?

Which of the following is a drawback of collision theory?

The proper orientation of reactant molecules leads to bond formation.

Who put forward the collision theory of chemical reactions?

Effective collisions are those in which molecules must acquire the energy of activation.

Which of the following explains the increase in the reaction rate by a catalyst?

When a catalyst is involved in the collision between the reactant molecules, more energy is required.