Rate of Reaction

Question 1

what is rate of reaction measured in

Answer 1

M/s
Moles/litre per second

Question 2

Chemical reaction to occur

Answer 2

• Reactants must collide with enough kinetic energy
• Reactants must also collide with the correct orientation

Question 3

Factors that change rate

Answer 3

• Increase surface area
• Increase concentration of solution (pressure for gases)
• Increase temperature
• Add a catalyst

Question 4

Increase surface area

Answer 4

• Greater surface area means there is more surface for the reaction to occur at (more spots to collide)
• This increases the number of successful collisions which will increase the rate of reaction

Question 5

Increasing concentration

Answer 5

• Increasing concentration means there will be more particles present and therefore more places for collisions to occur
• Increasing the likely-hood of successful collisions, thus increasing rate of reaction

Question 6

Increasing Temperature

Answer 6

Increases the kinetic energy:
- more collisions happening as the particle are moving with more speeds
- higher kinetic energy when colliding increasing likely-hood of successful collisions

Question 7

Adding catalyst

Answer 7

• A catalyst is a substance that increases the rate of reaction without being consumed in the process
• Adding a catalyst lowers the activation energy of a reaction by providing an alternate reaction pathway
• With lower activation energy there is a higher chance of a successful collision

Question 8

Measuring rate of reaction

Answer 8

• mass gained/mass lossed graph
• the gradient of those graphs give the rate of reaction
• maxwell boltzman diagram (shows how many particles have the minimum kinetic energy to meet the eactivation energy)