kinetics

Question 1

activation energy

Answer 1

minimum energy required for reaction to occur

Question 2

give 1 reason why the reaction between H and Cl is very slow at room temp

Answer 2

particles have sufficient energy to react

Question 3

Why does an increase in pressure, also increase the rate of the reaction between H and Cl

Answer 3

more particles in given volume

collide more often

Question 4

Why does an increase in temp, also increase the rate of the reaction between H and Cl

Answer 4

many more molecules have energy greater than the activation energy

Question 5

Suggest one reason why a solid catalyst for a gas-phase reaction is often in the form of a powder

(1)

Answer 5

increases surface area

Question 6

explain how a catalyst works

(2)

Answer 6

provides an alternative route with a lower activation energy

Question 7

a) x and y axis of Maxwell-Boltzmann curve

b) area under the graph

c) why this curve starts at the origin

Answer 7

y- number of molecules
x- (molecular) energy

b) total number of molecules in the sample

c) no molecules have no energy

Question 8

With reference to the Maxwell-Boltzmann distribution, explain why an increase in temp increases the rate of a chemical equation

Answer 8

more molecules have sufficient energy to react

more successive collisions

Question 9

explain what must happen for a reaction to occur between molecules of 2 diff gases

(2)

Answer 9

collision with activation energy

Question 10

explain why a small increase in temp has a large effect on the initial rate of reaction

(2)

Answer 10

many more collisions with E > EA (energy greater than the activation energy)