Kinetics

Question 1

define successful collisions

Answer 1

a collision resulting in a reaction (a new product is formed)

Question 2

define frequent collisions

Answer 2

how often collisions happen

Question 3

define activation energy

Answer 3

the minimum amount of energy required for a successful reaction

Question 4

define rate

Answer 4

the change in concentration of a product/reactant per unit of time

Question 5

what is the 1st law of thermodynamics

Answer 5

energy cannot be created or destroyed, only transferred

Question 6

what are the 5 factors that affect the rate of reaction?

Answer 6

surface area
concentration
pressure
catalyst
temperature

Question 7

describe the maxwell-boltzman molecular energies graph?

Answer 7

y axis - particles
x axis - energy in kj mol-1
area under the curve = total particles
emp is under the peak
eav is a little futher away from the emp on the right side.
Ea is where the asymptote is

Question 8

explain the concentration graph in comparison to the maxwell-boltzman curve

Answer 8

increased concentration increases the number of particles within the same volume.
so more frequent collisions occur in a given time, so faster ROR

Question 9

explain the surface area graph in comparison to the maxwell-boltzman curve.

Answer 9

the graph does not change
smaller particles = more surface area
higher surface area = the same number of particles in the same energy
so more successful collisions in a given time, so faster ROR

Question 10

explain the pressure graph in comparison to the maxwell-boltzman curve

Answer 10

graph does not change
increased pressure = the same number of particles in less volume
so there a more frequent collisions in a given time, so faster ROR

Question 11

explain temperature in comparison to the maxwell-boltzman graph

Answer 11

increase in temperature = increase in kinetic energy
so ROR increases as particles collide more frequently
AND
many more have the required activation energy for a successful reaction

Question 12

what is a catalyst and explain how it works?

Answer 12

a catalyst increases the rate of reaction and it is chemically unaltered

it lowers the activation energy by providing an alternative reaction pathway

Question 13

explain the graph of a catalyst in comparison to the maxwell-boltzman curve

Answer 13

increased ROR because once the activation energy is lowered, more particles have the required activation energy, so there are more successful collisions.