kinetics

Question 1

four factors affecting rate of reaction

Answer 1

-pressure= more particles in a space and therefore most likely to be colliding in the space
-concentration= more particles -more likely to collide more frequently more likely to have kore successful collisions and therefore rate of reaction increases
-temperature = more energy for reactant particles to collide- successful collisions in the correct orientations
-surface area = more area for particles to collide on larger surface area to vol ration higher rate of reaction

Question 2

rate of reaction equation

Answer 2

amount of reactant used or amount of product formed / time taken

Question 3

collision theory

Answer 3

1)two pairs of reactant particles move towards each other
2)they collide and reform so that each pair joins with a member of a different pair ,the products
3)the new pairs move away from each other
4)the collision must also take place. between the parts of the molecules that will react -so orientation needs to be correct

Question 4

two factors hindering a reaction

Answer 4

1)activation energy
2)orientation

Question 5

activation energy

Answer 5

minimum amount of energy needed tor reactants particles to collide and start a reaction and form products

Question 6

transition state

Answer 6

if the particles have enough energy bonds will break

some bonds are in the process of being made some bonds are in the process of being broken

Question 7

larger activation energy means

Answer 7

-reaction will take place slowly at rtp as few collisions

Question 8

what increases rate of reaction

Answer 8

• high temperature-higher the temperature the more kinetic energy particles gain so more frequent successful reaction
  -catalysts
  -high conenctration- more particles meaning the p-robability of more frequent successful collisions are higher
  -high pressure
  -high surface area to volume ratio - higher area for particles to collide on