Unit 3 Controlling The Rate

Question 1

Why is it important to be able to control reaction rates?

Answer 1

To ensure process are
Economically viable(this will result in good yield of products and profits for the company)

Safe(the reaction does not progress too quickly potentially causing explosions)

Question 2

How can average rate and reaction rate be calculated?

Answer 2

Avarage = changequantity/changetime

Reaction = 1/t

Question 3

What is meant by collision theory?

Answer 3

Particles must collide to react but not all collisions are successful
There must be
Sufficient energy
Orientation must be correct

Question 4

Explain why for a chemical reaction to occur the reactant molecules must collide with enough energy?

Answer 4

To overcome the repulsive forces(caused by outer electrons)and start to break the bonds between atoms

Question 5

What is a activated complex?

Answer 5

High energy intermediate state that is established when bonds inside the reactent molecule are breaking and new bonds are forming

Question 6

Use collision theory to explain the effects of collision geometry on reaction rates?

Answer 6

For successful collision to take place the collision geometry must be right(reactent molecules must he facing right way) so activated complex can form

Question 7

Use collison theory to explain the effects of temp on reaction rates?

Answer 7

If temp is increased the particles have more kinetic energy and then move more quickly and particles collide more often with higher chance of successful collisions

Question 8

Use collision theory to explain the effects of concentration on reaction rates?

Answer 8

If conc of reactants is increased there will be more reactant particles moving and more successful collision’s and reaction rate is increased

Question 9

Use collision theory to explain the effects of the partial size on reaction rates?

Answer 9

<partical size of recatent we are increasing surface area
Smaller particle size provides a greater surface area that collions can take place on

Question 10

What is meant by activation energy?

Answer 10

Minimum energy required for reaction to occur

Question 11

If reaction has low activation energy will reaction be fast or slow?

Answer 11

Fast as lot of particals will have required energy