Rates

Question 1

Collision Theory

Answer 1

In order for a reaction to occur:

• Reactant particles most collide
• with sufficient energy( greater than activation energy)
• and correct orientation

Question 2

Maxwell- Boltzmann Distribution

Answer 2

Focus on the frequency of successful collisions

under curve= total number pf particles.

Question 3

Activation Energy

Answer 3

The minimum amount of energy required for a reaction to take place.

Question 4

Unit for reaction rate

Answer 4

M/s

Question 5

Factors affecting rates of reaction

Answer 5

• Changing the surface area of solid reactions
• Changing the temperature of the reactants
• Changing the concentration of a solution
• Changing pressure of the reactant gases
• Using a catalyst

Question 6

Surface Area

Answer 6

increasing the number of particles available to react
increasing the frequency of collisions
increasing the frequency of successful collisions
increasing rate of reaction

Question 7

Increasing Temperature

Answer 7

• The average kinetic energy of particles is increased
• Greater propotion of particles having energy equal to or greater than the activation energy
• higher proportion of collisions being successful
• higher frequency of successful collisions
• rate of reaction increases.

Question 8

Increasing concentration

Answer 8

• there is a higher number of particles per unit volume
• increase in collisions frequency
• greater frequency of successful collisions
• rate of reaction increases.

Question 9

Catalysts

Answer 9

reduce the overall activation energy
increasing proportion of collisions that are successful
increasing frequency of successful collisions
increasing rate of reaction.

Question 10

Pressure

Answer 10

increasing frequency of successful collisions bc more particles per unit volume

Question 11

decrease in volume

Answer 11

increase in pressure

Question 12

increase in volume

Answer 12

decrease in pressure

Question 13

Dynamic equillibrium

Answer 13

a situation in which the rate of reaction of the forward and reverse reactions are equal, resulting in no observable changes overtime.

Question 14

Maxwell-Boltzmann Distribution

Answer 14

a graph showing the distribution of energy across a sample of particles.

Question 15

Reversible reaction

Answer 15

a chemical reaction that occurs in either the forward or reverse direction, given the appropriate conditions.

Question 16

closed system

Answer 16

no substances can escape or be added.

Question 17

yeild

Answer 17

the amount of product produced.

Question 18

Le Chatelier’s principle

Answer 18

a system at equilibrium has a tendency to partially oppose disruption.

Question 19

Position of the equilibrium

Answer 19

an evaluation of the relative amount of products compared to reactants, at equilibrium

Question 20

Haber process

Answer 20

the industrial production of ammonia 
with:
- 400-450 degree temp
-200atm pressure
-iron catalyst 
-1:3 N:H