rate of reaction

Question 1

actual yeild

Answer 1

refers to how much product was produced in the reaction
- influenced by temperature, pressure and concentration

Question 2

theoretical yield

Answer 2

refers to the maxiumum product possible

Question 3

transition state

Answer 3

• refers to when activatione nergy is absorbed
• new unstable arrangement of bonds are fomred
• bonds of reactants have been broken an new bonds are forming

Question 4

collision theory

Answer 4

for a reaction tor occur particles must
- collide with each other
- collide with sufficient energy to break the bonds in the reactants (fruitful collisions)
- collide with the correct orientation to break the bonds in the reactants

Question 5

increasing surface area of a reactant example answer

Answer 5

powder has smaller particles than chips
tha same mass of powder has a larger surface area than the chips
the larger area increases the frequency of collisions between particles and hence the rate of reaction

Question 6

increasing concentration of reactant example

Answer 6

a higher concentration of something means that, on average, the distance between particles is shorter than a lower concentration
the reduced distance between particles increase the frequency of collisions between particles and hence the frequency of successful collisions also increase.
the increase frequency of successful collisions increase the rate of reaction

Question 7

increasing the temperature of reaction

Answer 7

the higher temperature in the beaker means that, on average, the particles are moving faster and have a higher kinetic energy.
the faster movement increases the frequency of collisions
the higher kinetic energy increases the proportion of collision that occur with energy greater than the activation energy for the reaction.
these two factors increase the frequency of successful collisions and hence the rate of reaction.

Question 8

adding a catalyst

Answer 8

the use of a catalyst as a catalyst lowers the activation energy for the reaction providing an alternative reaction pathway
lowering the activation energy increases the proportion of collisions that occur with energy greater than the activation energy for the reaction
hence, the frequency of successful collisions and rate of reaction

Question 9

ways of measuring reaction rate

Answer 9

mass of gas over time
ph of reaction over time
colout over time
average rate = change in product/change in time

Question 10

factors that affect frequency of successful collisions

Answer 10

SA, temp, concentration,, catalyst

Question 11

factors affecting proportion of collisions

Answer 11

temperature, catalyst

Question 12

what to included at the start of every use collosion theory

Answer 12

“A successful collision occurs when particles collide with energy greater than equal to EA and in the correct orientation.”