Rate Equations - Physical 2

Question 1

Define the term rate of reaction

Answer 1

Change in concentration (of any reactant or product) per unit time. State what is being monitored (usually production of a product)

Question 2

At a given instant, how could you calculate the rate of reaction?

Answer 2

Rate of reaction = change in concentration / change in time

Question 3

How could you measure the rate of reaction experimentally (different methods)?

Answer 3

Use a colorimeter at suitable intervals if there is a colour change.
If gas is evolved, use a gas syringe to collect volume of gas evolved, or measure the change in
mass of the reaction mixture.

Question 4

How would you measure reaction rate for really fast reactions?

Answer 4

Use a flash of light to break bonds, use probe flashes to record amount of light absorbed by a species; this can show its concentration. First used for ClO2 → ClO* + O*.
Can now monitor reactions that occur in times as fast as 10-12 seconds

Question 5

How can you determine the rate constant and rate expression for a reaction?

Answer 5

Only experimentally

Question 6

What affects the value of the rate constant for a given reaction?

Answer 6

Temperature, nothing else

Question 7

Define the term order of a reaction with respect to a given product.

Answer 7

The power to which a species’ concentration is raised in the rate equation.

Question 7

Write a generic rate expression and state what each term means

Answer 7

Rate = k [X]x [Y]y;
k = rate constant for the reaction
[X] and [Y] are concentrations of species X and Y respectively x and y are the orders of reaction with respect to X and Y

Question 8

Do species need to be in the chemical equation to be in the rate expression?

Answer 8

No - species in the chemical equation may be excluded and species not in the chemical equation e.g. catalysts, may be included

Question 9

Define the term overall order of reaction.

Answer 9

The sum of the orders of reaction of all species in the rate expression e.g. (from earlier), total order =x+y

Question 10

How would you calculate the units of the rate constant?

Answer 10

Units of rate are moldm-3s-1 and units of concentration are mol dm-3
Rearrange rate equation to get k= Sub in units and cancel them out

Question 11

How would you draw a rate concentration graph?

Answer 11

Plot [A] against time, draw tangents at different values → draw a secondary graph of rate against [A]

Question 12

Draw a rate concentration graph for a zero order reactant.

Answer 12

check

Question 13

Draw a rate concentration graph for a first order reactant

Answer 13

check

Question 14

Draw a rate concentration graph from a second order reactant.

Answer 14

check

Question 15

How could you confirm that this reactant was second order? - check picture

Answer 15

Graph of rate against concentration squared would be a straight line through the origin - check pictures

Question 16

How could you find the rate expression using the initial rate method?

Answer 16

Do a series of experiments, during which you vary concentrations, so the concentration of just one reactant changes each time.
Plot a graph of concentration against time for each reactant and use a tangent at t=0 to find the initial rate of reaction.
Compare rates and concentrations between each experiment to find order of reactants and overall rate equation

Question 17

What must you add to react with the I2 as it is produced for an iodine clock reaction? (equation)

Answer 17

Known moles of sodium thiosulfate and a little starch; Reacts with I2 in 1:2 ratio
I2 + 2S2O32- → S4O62- + 2I-

Question 18

When does the starch turn a blue-black colour in an iodine clock reaction and why?

Answer 18

When all of the Na2S2O3 has been used up and so I2 is produced, which reacts with starch, leading to a blue black colour

Question 19

How can you calculate the rate of reaction from the data from an iodine clock reaction?

Answer 19

Record time taken for colour change to occur. Use rate = 1/t. This is effectively the initial rate

Question 20

What is the effect of a 10K temperature increase on the rate of reaction, roughly?

Answer 20

Doubles rate of reaction

Question 21

What is true of the half life of a first order reactant (concentration against time graph)?

Answer 21

Half life is constant

Question 22

What is the Arrhenius equation? What does each term mean?

Answer 22

check

Question 23

How can you convert the Arrhenius equation into a useful form for plotting a graph?

Answer 23

ln k= -Ea/RT + ln A
Graph of lnk against 1/T is a straight line: gradient = -EA/R and y intercept is lnA

Question 24

What is the rate determining step?

Answer 24

The slowest step in a reaction mechanism, which determines the overall rate of reaction

Question 25

How does the rate determining step link to the species involved in the rate expression?

Answer 25

Any species involved in the rate determining step appear in the rate expression. Species only involved after the rate determining step do not appear in the rate expression