Rates Of Reaction

Question 1

if you increase the pressure of a gasses reaction what happens to the rate of reaction? and why?

Answer 1

the rate or reaction increases, as there are more particles in a given area, so more chance of successful collisions.

Question 2

what is needed for a successful collisions?

Answer 2

Ea (activation energy)

Question 3

what are 3 ways to measure rates of reaction?

Answer 3

1. measure how long it takes for a certain volume of gas to be produced.
2. measure loss in mass over time.
3. disappearing cross if a solid is produced.

Question 4

what is the definition of activation energy?

Answer 4

minimum amount of energy required for a reaction to occur

i.e a successful collision.

Question 5

what 4 factors affect the rate of reaction?

Answer 5

surface area
concentration/ pressure
Temperature
catalyst

Question 6

what is a catalyst (definition)

Answer 6

speeds up a reaction but is chemicals unchanged at the end.

provides an alternative pathway.

Question 7

what happens in terms of the rate of a reaction throughout the reaction?

Answer 7

it’s the fastest at the start bust begins to slow as the limiting reagent starts to get used up (name it(the 1 not in excess)) then the reaction stops when it is used up.