Kinetics

Question 1

Definiton of activation energy

Answer 1

The minimum energy that a particle needs in order to react; the energy difference between the reactants and the transition state.

Question 2

What is collision theory

Answer 2

Reactions can only occur when particles collide with sufficient energy and in the correct orientation.

Question 3

Why do most collisions fail to cause a reaction?

Answer 3

Particles do not collide with sufficient energy/ correct orientation

Question 4

Describe the Maxwell-Boltzmann Curve

Answer 4

The energy on the x-axis

Number of particles on the y-axis

Question 5

Describe how Maxwell-Boltzmann curve changes for different temperature

Answer 5

Lower temperature: sharper peak at lower energy

Higher Temperature: Broader peak at higher energy

Question 6

Why does a small increase in temperature cause a large increase in the rate of reaction

Answer 6

Broad peak shows particles on average have more energy

And, a greater proportion of particles have E_a

Question 7

Describe the effect of change in conc on the rate of reaction in terms of collision theory.

Answer 7

A greater proportion of molecules which can react in the same volume.

Reactive particles are more tightly compacted so more likely to collide.

Question 8

Describe the effect of change in pressure on the rate of reaction using collision theory

Answer 8

Increase in rate as pressure increases due to A greater proportion of molecules which can react in the same volume.

And particles are more tightly compacted so more likely to collide.

Question 9

Effect of increase in temp on the rate of reaction using collision theory.

Answer 9

Increases speed of molecules which increases the likelihood of collision and energy of the particles when they collide.

Question 10

Describe how a catalyst increases the rate of a reaction

Answer 10

Provides an alternate path for the reaction which requires less activation energy.