Kinetics

Question 1

What is Collision theory?

Answer 1

For a reaction to take place particles must collide with enough energy to break bonds and at the right orientation

Question 2

What factors effect the rate of reaction and why?

Answer 2

-Increase in temperature: Increases the Ke meaning particles collide more frequently and with a higher energy
-Increase the conc of a solution: more particles means there are more collisions however graph will decline as there are less particles to react further into the reaction
-Increase in pressure: same effect as conc but with a gas
-Increase in surface area: more particles are available to collide
-Catalyst: provides an alternate pathway for reaction that has a lower activation energy

Question 3

Where are the particles with the highest energy on the Maxwell-Boltzmann distribution?

Answer 3

The right hand side of the curve

Question 4

Where are the particles with the most probable energy on the Maxwell-Boltzmann distribution?

Answer 4

At the peak of he curve

Question 5

How does a higher temperature effect the Maxwell-Boltzmann graph?

Answer 5

The curve becomes lower and moves to the right. The number of high energy particles increases.
(The area under the graph always remains the same as it represents he no. of particles)

Question 6

How will a Catalyst effect a Maxwell-Boltzmann graph?

Answer 6

Has no effect only the line for activation energy shifts to the left, as the activation energy decreases therefore more particles have the energy.

Question 7

Describe the structure and function of a catalytic converter?

Answer 7

They reduce the number of polluting gases as they react with the platinum and rhodium which coat the ceramic honeycomb structure thus has a large surface area meaning less expensive meals are needed. E.g CARBON MONOXIDE AND NITROGEN OXIDES ARE CONVERTED INTO CARBN DIOXIDE AND NITROGEN