Brainscape's Knowledge GenomeTM

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


See full index

Introductory Chemistry 2 (CHM121) > Solutions, Solubility and Thermodynamics > Flashcards

Solutions, Solubility and Thermodynamics Flashcards

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

Solution

A

A homogeneous mixture containing particles the size of a typical ion or covalent molecule. (0.1–2.0 nm in diameter)

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

Colloid

A

A homogeneous mixture containing particles with diameters in the range 2–500 nm

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

Suspensions

A

Mixtures with even larger particles, but they are not considered true solutions because they separate upon standing

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

Solute

A

The dissolved substance in a solution

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

Solvent

A

The major component in a solution

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

Solubility

A

The maximum amount of solute that can dissolve in a specific amount of solvent usually 100 g.

g of solute / 100 g water

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

A solution is saturated when…

A

…no additional solute can be dissolved at a particular temperature

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

A Supersaturated solution can form when…

A

…more than the equilibrium amount of solute is dissolved at an elevated temperature, and then the supersaturated solution is slowly cooled.

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

An Unsaturated solution is formed when…

A

more of the solute can dissolve in it at a particular temperature.

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

What is the condition for crystallisation?

A

For crystallisation to occur, the molecules or ions of solute must arrange themselves properly to form crystals.

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

Factors affecting solubility…

A 
Solute-solvent interaction
Temperature effect (Solid and Liquid)
Pressure effect (Gases)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is the relationship between the solubility of gases and their sizes?

A

Solubility of gases increases with size of gas due to London dispersion force

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

Temperature and Solubility of Solids

A

The solubility of most solids increases with an increase in the temperature

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

Temperature and Solubility of Gases

A

The solubility of gases decreases with an increase in temperature.

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

Relationship between solubility and pressure

A

Pressure has little effect on the solubility of liquids and solids. The solubility of gases is strongly influenced by pressure. Gases dissolve more at high pressure.

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

What does Henry’s law show?

A

The relationship b/w pressure and the solubility of a gas

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

According to Henry’s law, what does the solubility of a gas in a liquid depend on?

A

Temperature
The partial pressure of the gas over the liquid,
The nature of the solvent,
The nature of the gas.

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

State Henry’s law

A

At constant temperature the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas in equilibrium
Cg= khPg

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

What are the conditions for Henry’s law?

A

Molecules are at equilibrium.
Gases not at high pressures (e.g., N2(g) asupply)
No chemical reaction between the solute and solvent

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

When do deviations from Henry’s law become noticeable?

A

As concentrations and partial pressures increase, deviations from Henry’s law become noticeable.

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

What are solutions which are found to obey Henry’s law called?

A

Ideal dilute solutions

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

How does antifreeze work?

A

The added solute also raises the boiling point of the solution above that of pure water, making it possible to operate the engine at a higher temperature.

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

What are colligative properties?

A

Colligative properties are physical properties of solutions that depend on the quantity (concentration) but not the kind or identity of the solute particles. Colligative properties depend on the collective effect of the number of solute particles.

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

Examples of colligative properties

A

Freezing-point depression
Boiling-point elevation
Vapor-pressure lowering
Osmotic pressure

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

What is vapour pressure?

A

The vapour pressure is the pressure exerted by the vapor when it is at equilibrium with the liquid (that is, when the rate of vaporization equals the rate of condensation).

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

How does vapour pressure determine volatility?

A

A substance that has no measurable vapor pressure is nonvolatile, whereas one that exhibits a vapor pressure is volatile.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Describe the formation of a solution of volatile and non-volatile components.

A

A solution consisting of a volatile liquid solvent and a nonvolatile solute forms spontaneously because of the increase in entropy that accompanies their mixing.

Therefore, when a nonvolatile solute is present, the vapor pressure of the solvent is lower than the vapor pressure of the pure solvent,

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

State Raoult’s law

A

It states that the partial vapor pressure exerted by solvent vapor above the solution, Psolution, equals the product of the mole fraction of the solvent, Xsolvent, times the vapor pressure of the pure solvent, P°solvent:

	Psolution = Xsolvent .  P°solvent
29
Q

What are the conditions for Raoult’s law?

A

Raoult’s law assumes that the solution is ideal. Therefore, the forces between solute and solvent molecules must be the same as the solvent to solvent.

30
Q

What is an ideal mixture?

A

An ideal mixture of two liquids will have zero enthalpy change of mixing.

31
Q

What is boiling point elevation?

A

If you add solute it will change the solvent’s vapor pressure, therefore the boiling point changes.

The Boiling point elevation, ΔTb, is directly proportional to the molality of the solution
ΔTb= Kbmsolute

32
Q

What happens with freezing point depression?

A

There are more atoms of pure solvent going from solid to liquid than from liquid to solid.

33
Q

Examples of ideal mixtures

A

hexane and heptane
benzene and methylbenzene
propan-1-ol and propan-2-ol

34
Q

What happens in a non-ideal solution?

A

Solute-solvent interactions are significantly different from solute-solute and solvent-solvent interactions

35
Q

Negative deviation from Raoult’s law

A
  • The vapor pressure of a mixture is lower than expected.
  • The adhesive forces between different components are stronger than the average cohesive forces between like components
  • Both components have a lower escaping tendency in the solution than in the pure liquids
  • Liquids mix exothermically.
36
Q

Positive deviation from Raoult’s law

A
  • Two liquids mix endothermically, this indicates that the solute-solvent interactions are weaker than the interactions among the molecules in the pure liquids.
  • The cohesive forces between like molecules are greater than the adhesive forces
  • Dissimilarities of polarity leads both components to escape solution more easily.
  • Vapor pressure is greater than expected from Raoult’s law.
37
Q

Examples of positive deviation from Raoult’s law

A

benzene and methanol
carbon disulfide and acetone
chloroform and ethanol

38
Q

Examples of negative deviation from Raoult’s law

A

chloroform and acetone

39
Q

What is chemical thermodynamics?

A

The chemistry that deals with energy exchange, entropy, and the spontaneity of a chemical process.

40
Q

Diathermal walls

A

The system and its surroundings are separated by walls of some kind. Walls that permit heat to flow through them, such as those of the engine block, are called diathermal walls.

41
Q

Properties of internal energy

A
  • The sum of all possible forms of energy in a system.
  • Cannot be measured, we can only measure changes in energy
  • Atoms, ions and molecules all possess internal energy
  • Independent of pathways used to reach the state
42
Q

State function

A

A property dependent only on the state of the system (i.e. what condition that system is in and not on the pathway)

43
Q

Examples of state functions

A

Pressure

Temperature

44
Q

If the products have more energy than the reactants …

A

…the change is positive

45
Q

If the reactants have more energy than the products …

A

…the change is negative

46
Q

What does Gibb’s free energy do?

A

G controls the position of equilibrium in closed systems at constant temperature and pressure

47
Q

Applications of thermodynamics

A 
Extraction, refining
Corrosion
Phase transformation-phase diagram calculation
Materials processing
Design of new materials.
48
Q

Types of thermodynamics systems

A

Open
Closed
Isolated

49
Q

Explain the term, phase.

A

The term, phase is used for that portion of the investigated system volume in which its proper ties are constant or continuously changing in space

50
Q

When does a thermodynamic process take place in a system?

A

If the properties of a system change in time, i.e. if at least one thermodynamic quantity changes, we say that a certain thermodynamic process takes place in the system.

51
Q

Types of thermodynamic processes

A

Reversible and Irreversible Processes
Processes at a constant quantity
Cyclic Processes

52
Q

What is a reversible process?

A

If a system is nearly at equilibrium in every moment, and that, consequently, the direction of the process may be reversed by even a very slight change of the initial conditions, the process is called reversible or equilibrium. A reversible process is thus a sequence of (nearly) equilibrium states of a system.

53
Q

What is an irreversible process?

A

A real world system is out of equilibrium at least at the beginning. These processes are called irreversible or non-equilibrium (the direction of the process cannot be reversed by any slight change of external conditions, and the process is a sequence of non-equilibrium states)

54
Q

Isothermal

A

Temperature

55
Q

Isobaric

A

Pressure

56
Q

Isochoric

A

Volume

57
Q

Adiabatic

A

Heat

58
Q

Isentropic

A

Entropy

59
Q

Isenthalpic

A

Enthalpy

60
Q

Polytropic

A

Heat capacity

61
Q

What is a cyclic process?

A

A cyclic process is such at which the final state of the system is identical with its initial state. In a cyclic process, changes of thermodynamic quantities are zero.

62
Q

What is a property?

A

Any characteristic of a system in equilibrium is called a property.
- vary directly with the size of the system
Examples: volume, mass, total energy
- are independent of the size of the system
Examples: temperature, pressure, color

63
Q

Types of properties

A

Extensive properties

Intensive properties

64
Q

Extensive properties

A

Vary directly with the size of the system.

Examples: volume, mass, total energy

65
Q

Intensive properties

A

Are independent of the size of the system

Examples: temperature, pressure, color

66
Q

Extensive properties per unit mass are…

A

…intensive properties, eg. Specific volume v = Volume/Mass = V/m, Density r = Mass/Volume = m/V

67
Q

Spontaneous Reaction-

-

A

A reaction that occurs under specific conditions, occurs without outside intervention.

68
Q

Non-spontaneous Reaction

A

A reaction that does not occur under specific conditions

Introductory Chemistry 2 (CHM121) (4 decks)

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