Kinetics

Question 1

Define activation energy

Answer 1

The minimum energy required before a reaction can occur. This is necessary to break the bonds within the reactants.

Question 2

What must particles do in order to react?

Answer 2

Collide with the necessary activation energy
Be in the correct orientation

Question 3

How does each factor impact a kinetics graph?

Answer 3

Temperature changes the slope
Concentration changes both
Volume changes the end point

Question 4

What is the Maxwell-Boltzmann distribution curve?

Answer 4

X = energy Y = number of molecules
Most probable energy, mean/average, activation energy
Starts at (0,0) as no particles have zero energy
Area under the graph = total number of molecules

Question 5

What does increasing the temperature do to the rate of a reaction?

Answer 5

Increases the rate
Particles move faster and many more successful collisions (increases the frequency of them)

Question 6

What does increasing the concentration do to the rate of reaction?

Answer 6

Increases the rate
More particles in a given volume
Means increased frequency of successful collisions

Question 7

What is a catalyst and what does it do?

Answer 7

Substance that speeds up a reaction without being used up/changed
Provides an alternative reaction pathway and lowers the activation energy

Question 8

How does increasing the temperature impact the Maxwell-Boltzmann distribution curve?

Answer 8

Moves the curve to the right and lower
Increasing the activation energy

Question 9

How does decreasing the temperature impact the Maxwell-Boltzmann distribution graph?

Answer 9

Shifts the curve to the left and higher
Lowers the activation energy

Question 10

How does a catalyst affect the Maxwell-Boltzmann Distribution graph?

Answer 10

No change to the curve
Activation energy does shift left