Brainscape's Knowledge GenomeTM

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


See full index

A level Chemistry > Unit 3.7 - Entropy and the feasibility of reactions > Flashcards

Unit 3.7 - Entropy and the feasibility of reactions Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

What term do we use if a reaction can happen?

A

Feasible

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

Spontaneous reactions

A

Reactions that happen easily, on their own accord without outside interference

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

Example of a spontaneous reaction

A

Group 1 + water

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

Examples of reactions that need happen (are feasible but not spontaneous)

A

Rusting
Food oxidations

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

Examples of reactions that are not feasible (don’t happen)

A

Platinum in water
Br2 + 2Cl-

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

What affects the feasibility of a reaction?

A

The change in energy - going down an energy gradient
The activation energy

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

What do both the change in energy and activation energy affect for a reaction?

A

Its feasibility

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

What type of reactions seem to be feasible and what type of reactions less so?

A

Feasible —> exothermic reactions
Less feasible —> endothermic reactions

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

Why are endothermic reactions not favourable?

A

Products are less stable than the reactants

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

Give 2 examples of spontaneous endothermic reactions

A

-sodium hydrogencarbonate and hydrochloric acid reacting in the cold
-ionic substances dissolving in water at room temperature

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

What type of reaction is diamond burning in oxygen?

A

Very exothermic

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

Diamond burning in oxygen is a very exothermic reaction, so why doesn’t it happen spontaneously?

A

The presence of strong covalent bonds in diamond means that it takes a lot of energy to break apart the carbon atoms in diamond in order to free them up to burn with oxygen = very high temperature needed

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

What is another factor that we need to determine whether a reaction is feasible, on top of just knowing the enthalpy change?

A

Entropy

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

What 2 things do we need to know in order to determine whether a reaction is feasible?

A

Enthalpy change
Entropy

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

Symbol for entropy

A

S

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

What is entropy?

A

A quantitative measurement of the freedom of molecules - a measure of disorder

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

S meaning

A

Entropy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Units of entropy

A

JK-1mol-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Name and explain the 3 things that affect the value of entropy

A

The more disordered a substance, the higher the entropy
Temperature
Entropy will also generally be higher if there are more moles or more complicated molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What does a more disordered substance do to the value of the entropy?

A

Increases it

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is another thing that increases entropy except for being a disordered substance?

A

Entropy will generally be higher if there are more moles or more complicated molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

example of entropy increasing for a more complicated molecule

A

CO2>CO in terms of entropy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Put solid liquid and gas in order of increasing entropy

A

S (solid) < S (liquid) < S (gas)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

why do solids have low entropy values?

A

Highly ordered particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Why do gases have the highest entropy values?

A

Most disorganised particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Why does a liquid have an intermediate entropy value?

A

Less ordered particles than a solid, but not as disorganised as the particles of a gas

27
Q

What does the superscript o symbol mean?

A

Under Standard conditions

28
Q

What does a substance being more complex make it?

A

More entropic

29
Q

What type of compounds are the most entropic?

A

More complex ones

30
Q

Is air quite entropic? Why?

A

Yes, since it’s composed of a mixture of different gases (complex)

31
Q

What does each substance at a given temperature and pressure have?

A

A unique entropy

32
Q

How do we work out the entropy change for a reaction?

A

Change in entropy = entropy of all the products - entropy of all the reactants

33
Q

How can we predict whether entropy will increase or decrease without entropy values?

A

By counting the number of moles of elements in their different states and remember that S(solid)<S(liquid)<S(gas)

34
Q

Stages to working out entropy changes

A
  1. Write a balances equation to check number of moles
  2. Work out entropy of products and reactants (remembering to multiply up by the number of moles)
  3. Use the equation: change in entropy = entropy of all the products - entropy of all the reactants
  4. CHECK: entropy has increased - we could predict this as a single solid has produced two substances, a solid and a gas
35
Q

What is the entropy change if entropy increases?

A

Positive

36
Q

What does a positive entropy change mean has happened?

A

The entropy has increased

37
Q

Second law of thermodynamics

A

For a reaction to be feasible, the total entropy of the system has to increase, so ΔS must be positive

38
Q

What conditions have to be true in terms of the entropy of the reaction for a reaction to be feasible?

A

For a reaction to be feasible, the total entropy of the system has to increase, so ΔS must be positive

39
Q

What does the change in entropy have to be for the reaction to be feasible?

A

Positive

40
Q

What has to happen to the total entropy of a reaction for the reaction to be feasible

A

Has to increase

41
Q

When will entropy always tend to increase during a reaction?

A

In any isolated system that is not in equilibrium

42
Q

Explain why the entropy will always tend to increase in any isolated system that is not in equilibrium

A

This is the overall entropy - in different parts of the system, the entropy may decrease, but this is because it has increased in other parts of the system
This includes the entropy change of the surroundings

43
Q

What does the overall entropy include?

A

The entropy change of the surroundings

44
Q

NaCl (s) —> Na+ (aq) + Cl- (aq) ΔHsolultion = +5kJmol-1
For any ionic substance to dissolve in water, the enthalpy change of solution must be exothermic, so why does this salt dissolve in water?

A

Since there’s an increase in entropy of the system
Therefore, the total entropy of the system is positive
(aq = more disordered than s = increased entropy)

45
Q

What two things do we need to soldier to work out if a reaction is feasible at a certain temperature?

A

Need to consider the enthalpy change of the reaction and the change in entropy

46
Q

Gibbs free energy equation

A

ΔG = ΔH - (TΔS)

47
Q

What must ΔG be for a reaction to be feasible?

A

Negative

48
Q

ΔG meaning

A

Gibbs free energy

49
Q

Units of everything in the Gibbs free energy equation

A

ΔG = Gibbs free energy in kJmol-1
ΔH = enthalpy change in kJmol-1
ΔS = entropy change in JK-1mol-1
T = temperature in K

50
Q

Which value do we need to alter in the Gibbs free energy equation and why and how?

A

Entropy change
In JK-1mol-1
Need it to be consistent, so need to divide it by 1000

51
Q

What could we be asked in terms of the Gibbs free energy equation?

A

If a reaction if feasible at a given temperature
At which temperature the reaction becomes feasible

52
Q

What value does Gibbs free energy have to be for a reaction to take place?

A

Less than or equal to zero

53
Q

How do we calculate the temperature at which a reaction can take place?

A

ΔG = O
So TΔS = ΔH
T = ΔH/ΔS

54
Q

How do we know which reaction is the most feasible out of two values?

A

The most negative Gibbs free energy value

55
Q

What does the value of ΔG having to be for a reaction to occur spontaneously?

A

Negative

56
Q

If ΔG is negative, what does the reaction do?

A

Happens spontaneously

57
Q

If ΔG is positive, what does the reaction do?

A

Doesn’t occur spontaneously

58
Q

How do we know when a reaction will not occur spontaneously?

A

When ΔG is positive

59
Q

What are the two conditions that we can use to prove whether or not a reaction is feasible?

A

ΔG must be negative
The total entropy of the system has to increase so ΔS must be positive

60
Q

When do we use the total entropy of the system increasing for a reaction to be feasible explanation on why a reaction has occurred?

A

When we only have information about the states of the elements since we can work out whether entropy has increased/decreased from this

61
Q

When do we use the fact that ΔG needs to be negative for a reaction to be feasible to prove why a reaction has occurred?

A

When we have information about ΔG

62
Q

If the value for the Gibbs free energy of a reaction isn’t negative (and so isn’t feasible), what may be done to attempt to make the reaction occur spontaneously with no interference (make it feasible)?

A

The temperature may be increased

63
Q

What’s the best method for working out whether a reaction is feasible when we have a solution reaction? Explain

A

Electrochemical data (Ecell) since Gibbs free energy data is for solids and liquids. We should be using standard conditions of concentration 1moldm^-3 and 298K temperature too.

64
Q

What do we need to remember to with entropy changes?

A

Multiply up molar ratios

A level Chemistry (39 decks)

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