Rates of reaction

Question 1

What is collision theory?

Answer 1

for a reaction to occur between particle they must collide. The collision provides the energy needed for the reaction to take place

speed at which a reaction occurs is directly prop to no. ccollisions per unit time and the amount of effective collisions

Question 2

define effective collisions?

Answer 2

A-collision which results in a reaction that produces one or more products

Question 3

factors that affect rate of reactions .

Answer 3

Temperature
Concentration
Surface area
pressure
catalysts
nature of reactantS

Question 4

give afull explanation of how each factor affects the rate of reaction.

Answer 4

increase kinetic energy etc-

Question 5

Measuring rate of reaction formulae :

Answer 5

change in conc Of reactants÷ time

change in conc.of products ÷ time

Question 6

Activation energy ?

Answer 6

Minimum amount of energy needed for a chemical reaction to take place

Colliding Molecules must have kinetic energy greater then or = to the activation energy in order for the collision to be successful

The more mOlecules that have enough energy, the faster the rate of reaction

Question 7

enthalpy equation?

Answer 7

change in H = E products - E reactants

Question 8

Effects of a catalyst ?

Answer 8

> takes part in reaction but doesnt get used up
> dont cause a reaction
> create alternate paths for reaction
> lower act. energy
> dont charge H
> don't affect amount of product formed

Question 9

Rate of reaction measured practically?

Answer 9

> record charge in mass of reaction vessel
record volume of gas produced → gas syringe
Colour change or precipitate formation

Question 10

heat of reaction?

Answer 10

energy absorbed or released by a chemical reaction

Question 11

activated complex ?

Answer 11

Unstable state between being a product and reactant