rate of reactions

Question 1

1st main method used to measure rate of reaction

Answer 1

how quickly reactants are used up or rate of disappearance of product

Question 2

2nd main method used to measure rate of reaction

Answer 2

how quickly the product are formed or rate of appearance of product

Question 3

formula

Answer 3

rate of reaction = amount of reactant used OR amount of product formed / time

Question 4

common ways to measure rate of reaction experimentally

Answer 4

precipitation, change in mass, volume of gas given off

Question 5

collision theory

Answer 5

• in a chemical reaction a collision is involved between reactant particles
• states that molecules must collide with sufficient energy (AE) and with suitable orientation to disrupt the bonds

Question 6

collision theory applied to concentration

Answer 6

• if solution is more concentrated, there is greater density of reactant particles meaning there more collisions
• bc at the same proportion there is greater rate of collision
• greater rate of successful collisions

Question 7

collision theory applied to subdivision

Answer 7

• by increasing surface area, we are exposing more of the reactant
• more reactant particles are available for collision
• higher successful collision rate
• faster reaction time

Question 8

collision theory applied to temperature

Answer 8

1- reactant particles are moving faster meaning rate of collision increases
- increase of successful collision and faster reaction time
2- increasing temp effect molecular energies of reactants
- reactant have sufficient kinetic energy to supply AE needed for reaction
- successful collision and faster rate of reaction

Question 9

catalyst

Answer 9

substance that speeds up a chemical reaction but is not used up in the reaction

Question 10

collision theory applied to catalyst

Answer 10

• provides alternative pathway for the reaction than the one available with the reactant alone
• lower AE meaning less collision energy is required