Week 8: Reaction kinetics and reversible reactions

Question 1

For 0th reaction order what is the rate equation?

Answer 1

(60a)

Question 2

For 1st reaction order what is the rate equation?

Answer 2

(60b)

Question 3

For 2nd reaction order what is the rate equation?

Answer 3

(60c)

Question 4

For 3rd reaction order what is the rate equation?

Answer 4

(60d)

Question 5

For nth reaction order what is the rate equation?

Answer 5

(60e)

Question 6

For 0th reaction order what is the integrated expression?

Answer 6

(60a)

Question 7

For 1st reaction order what is the integrated expression?

Answer 7

(60b)

Question 8

For 2nd reaction order what is the integrated expression?

Answer 8

(60c)

Question 9

For 3rd reaction order what is the integrated expression?

Answer 9

(60d)

Question 10

For nth reaction order what is the integrated expression?

Answer 10

(60e)

Question 11

For 0th reaction order what is the half-life?

Answer 11

(60a)

Question 12

For 1st reaction order what is the half-life?

Answer 12

(60b)

Question 13

For 2nd reaction order what is the half-life?

Answer 13

(60c)

Question 14

For 3rd reaction order what is the half-life?

Answer 14

(60d)

Question 15

For nth reaction order what is the half-life?

Answer 15

(60e)

Question 16

For 0th reaction order what are the units of k?

Answer 16

(61)

Question 17

For 1st reaction order what are the units of k?

Answer 17

(61)

Question 18

For 2nd reaction order what are the units of k?

Answer 18

(61)

Question 19

For 3rd reaction order what are the units of k?

Answer 19

(61)

Question 20

For nth reaction order what are the units of k?

Answer 20

(61)

Question 21

Why in a state of equilibrium, do the concentrations of reactants and products no longer change with time?

Answer 21

Because under such conditions, all reactions are microscopically reversible.

Question 22

What is the process of approaching equilibrium?

Answer 22

Rate equation
Initial condition
Mass balance condition
Introduce normalised variables
Rate equation in normalised form
Solution produces the concentration expressions
Reaction quotient Q
Equilibrium is Q at infinite time

Question 23

Derive the approach to equilibrium.

Answer 23

(62)

Question 24

What is the difference between the reaction quotient Q and equilibrium constant K?

Answer 24

Approach to equilibrium Q<theta

At equilibrium Q = k = theta

Question 25

What does k+ denote?

Answer 25

The forward rate constant

Question 26

What does k- denote?

Answer 26

The reverse rate constant

Question 27

What is the equilibrium constant?

Answer 27

Relates to the relative preference for the chemicals to be in the combined state C compared to the disassociated state. Keq = k- / k+ Has units of concentration

Question 28

What does it mean if keq is small?

Answer 28

There is a high affinity between A and B.