Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

DS1101 - S1 Y1 > Week 4 - Kinetics > Flashcards

Week 4 - Kinetics Flashcards

1
Q

Where is kinetics used in dentistry

A
  • kinetics of resin composites and how fast they set
  • degradation kinetics of API in drugs (how they store)
  • enzyme suppression treatment designed to reduce pocket depth
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What does kinetics refer to

A

How fast a reaction proceeds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what is rate constant k (lowercase)

A
  • indicated how fast a reaction is e.g. k=10^5
  • indicates the time to get to equilibrium
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is Kc

A

Equilibrium constant - ratio of the concentrations of the products and reactants - can only be measured at equilibrium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the units for the rate (k)

A

mol/Ls
Moles per liter seconds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What are elementary steps

A

In chemical reactions the ‘real process’ occurs in elementary steps, where the sum of the elementary steps to give the balanced equation.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What does RDS stand for

A

Rate determining step

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the RDS

A

The the elementary step in a chemical reaction which requires the highest amount of energy (has the larger energy barrier for it to react) and it determines the rate law.
The slowest step, which determines the overall rate and molecularity of the reaction.

The rate determining step is the slowest elementary step of a chemical reaction it determines the overall rate and molecularity. The RDS is the elementary step with the largest energy barrier (activation energy). It is also used to determine the rate law as it is the slowest elementary step in the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is the Molecularity of a step

A

The number of reactants in an elementary step
E.g.
A –> B = unimolecular
C + B –> D = Bimolecular RDS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is an intermediate

A

Species which is produced in the middle of a multi step reaction.

It is the lowest point in energy between two consecutive elementary steps. The reaction intermediate is located as the ‘dip’ between two elementary steps within the reaction and is a species which appears in the mechanism of a reaction but not in the final balanced equatio

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are reaction orders

A

The coefficient of the reactants determines reaction order. E.g. [A]^1 = first order with respect to A

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is a first order reaction

A

when the rate changes proportionally with the concentration of the reagent (1 for 1)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is the overall reaction order/ overall molecularity

A

the sum of all of the individual orders

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q
A

Reactants

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q
A

Transition state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q
A

Products

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is the effects of temperature on the rate of reaction

A

Temp Increase
- Increases the number of particles with sufficient activation energy
- Increases the kinetic energy of the particles hence increasing the number of successful collisions
- increases overall rate of reaction

18
Q

What is this equation and what do the letters stand for

A

ArrheniT = temperature in kelvin
R = Gas constant
Ea = activation energy (J/mol)
e = exponential
k = reaction constant
A = frequency factor us Equation

19
Q

What are the units for activation energy

A

J/mol

20
Q

Impact of high activation on rate

A

High Ea = small k (by Arrhenius equation = slow rate of reaction

21
Q

What is the rough rule for change of temperature on rate

A

For reactions happening at room temperature the rate of reaction doubles for ever 10 degrees rise in temperature

22
Q

What is the initial rate

A

rate of reactions at the very beginning of the reaction

23
Q

What is the instantaneous rate

A

rate of reaction at any specific point in time hence it will always be different depending on what time you measure it - changes all the time until equilibrium

24
Q

What is the average rate

A

the average rate of reaction over the whole reaction

25
Q

What does this equation let you calculate

A

Differential Rate Law
The rate at a specific moment (instantaneous)
where d = delta (change in)
where there’s a -1 since the rate is a decrease in reactants over time

26
Q

What does this equation let you find

A

General Rate Law
Lets you predict the rate of the reaction when provided with the concentrations

27
Q

What does this equation let you find

A

Integrated Rate Law
Lets you calculate the rate over the period t, used to work out changes in concentrations or how long a reaction will take
*will mainly focus on first order reactions

28
Q

What does this equation let you find

A

Half life

29
Q

What are catalysts and their function

A

Catalyst are reagents added to a reaction in non-stoichiometric amounts
They
- increase the rate of reaction
- Lower Ea for RDS
- Are not consumed after a reaction
- Don’t affect K/ the yield

Catalyst provide a different pathway for a reaction to occur which reduces the activation energy of the reaction

30
Q

What are homogeneous catalysts

A

Catalyst in the same phase/state (solid, liquid) as the reactants

31
Q

Example of a homogenous catalyst

A

used in production of acetic acid

32
Q

What are heterogeneous catalysts

A

Catalyst in different phases/state (solid, liquid) to the reactants

33
Q

Example of a heterogeneous catalyst

A

catalytic converter (solid catalyst) in car exhaust (reactant gases)

34
Q

What is a pharmaceutical drug

A

A pharmaceutical or drug is some sort of dosage aimed to diagnose, cure, treat or prevent a disease. They are most commonly seen as tablets (compressed solids)

35
Q

What is the composition of a tablet

A

5 - 10% = Active Pharmaceutical Ingredient
80% = Fillers, disintegrants, lubricants, colorants, flavours
10% = Substances that change the nature of the delivery of the API
e.g. compounds which ensure easy disintegration if it needs to move very quickly.
e.g. May be coated to make it acid resistant so it can make it through the stomach

36
Q

What is an API

A

Active Pharmaceutical Ingredient - which is the biologically active substance in drug, typically a small organic molecule
- some medications may contain more than one API and APIs from different medications can interfere with each other often resulting in severe complications

37
Q

What should you consider with API

A
  • some medications may contain more than one API
  • APIs from different medications can interfere with each other often resulting in severe complications
38
Q

What may cause Pharmaceutical drug decomposition

A
  • Light (photodegradation)
  • Heat (thermal)
  • Redox (oxidation)
  • Water (hydrolysis)
39
Q

How do you calculate the shelf life of a drug

A

Half life where (90% is remaining
In(9/10)/k = 0.105/k

40
Q

What is pharmacokinetics

A

Study of the time line of the drug when it is delivered till when it is removed from the body.
Tracts the adsorption, bioavailability, distribution, metabolism and excretion of the drug

DS1101 - S1 Y1 (63 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions