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Chemistry > Solutions > Flashcards

Solutions Flashcards

1
Q

What is required for a chemical reaction to take place?

A

Collision energy: activation energy, the minimum value of energy required for the reaction to take place
Collision geometry: modules must collide with the correct orientation

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2
Q

What is a exothermic reaction?

A

Reaction where heat/energy is released

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3
Q

What is needed for an exothermic reaction to take place?

A

Need to give it a bit of energy

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4
Q

How much energy will the product of an exothermic reaction have?

A

Less than what it started out with

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5
Q

How much energy will the product of an endothermic reaction have?

A

More energy than the reactants

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6
Q

Which have higher activation energy, exothermic or endothermic reactions?

A

Endothermic reactions

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7
Q

What factors affect rate of reaction?

A

Temperature: increase increases rate of reaction as particle kinetic energy is increased
Concentration: increase increases rate of reaction due to increase in correctly oriented collisions
Particle size: decrease in size increases rate of rector due to increase in surface area
Pressure ( only gasses) & volume: increase pressure or decrease volume increases rate of reaction
Catalyst: reduces activation energy

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8
Q

Definition of equilibrium

A

At equilibrium the rate of the forward reaction = the rate of the reverse reaction

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9
Q

What are the conditions for equilibrium reactions?

A

They are dynamic
Must occur in a closed system
Concentrations must be constant
No macroscopic changes take place

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10
Q

What is the equilibrium constant?

A

Constant value for a certain reaction at a certain temperature

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11
Q

Formula for equlibrium constant

A

Google the answer

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12
Q

What is importat to remember when calculating equilibrium constant?

A

Units

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13
Q

How do you figure out what direction a reaction will favor?

A

Calculating the possible equilibrium constant. If it is lower the one given the forward reaction wil be favored, if it is high the backwards will se favored

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14
Q

What are the 3 possibilities for the solution of Q in comparison to k?

A

Q = k, equilibrium
Q > k, reaction go left, reverse reaction is favored
Q < k, reaction go right, forward reaction is favored

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15
Q

What does Le Chatelier’s principle state?

A

If we change something in a reaction it will adjust so equilibrium is reached again

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16
Q

How does added reactants change the equilibrium?

A

Reaction goes right, forward reaction is favoured

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17
Q

How does added products change the equilibrium?

A

Equilibrium goes left, reverse reaction is favoured

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18
Q

How does increase in pressure (decrease in volume) change the equilibrium? (Gasses only )

A

Side with less molecules is favoured

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19
Q

How does decrease in pressure (increase in volume) change the equilibrium? (Gasses only)

A

Side with more molecules is favoured

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20
Q

How does increase in temperature of an endothermic change the equilibrium?

A

Increase in product, reverse reaction is favoured

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21
Q

How does increase in temperature of an exothermic change the equilibrium?

A

Decreases product & forward reaction is favoured

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22
Q

What happens to the equilibrium constant k when temperature is changed?

A

It changes as well

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23
Q

What is delta H in an endothermic reaction?

A

Positive

24
Q

What is delta H in an exothermic reaction?

A

Negative

25
Q

What effect does a catalyst have on the equilibrium?

A

It is reached faster, no effect on K (equilibrium constant)

26
Q

What is a homogenous mixture?

A

Uniform mixtures, no distinguishable components
Ex : salt water

27
Q

What is a heterogenous mixture?

A

None uniform mixtures, distinguishable components
Ex: blood

28
Q

Definition of solution

A

Homogenous mixture of 2 or more substances

29
Q

What are the 2 components of a solution?

A

Solvent & solute

30
Q

What is the solvent?

A

The thing that dissolves the other substance, what takes up the volume, larger mass or more moles

31
Q

What is the solute?

A

The thing that gets dissolved

32
Q

What phases can solutions be?

A

Gas, liquid or solid

33
Q

Definition of solubility

A

The amount of solute that will dissolve per volume of solvent

34
Q

What does it mean when something has a higher solubility

A

More will be dissolved

35
Q

What is solubility impacted by?

A

Molecular structure: some chemicals dissolve more than others
Pressure (only for gas): increase in pressure increases gas solubility in a liquid
Temperature: increased temperature decreases gas solubility in liquid. Increases in temperature increases solid/liquid solubility in liquid

36
Q

Rule about solubility

A

Like dissolves like

37
Q

Will a polar solute dissolve in a polar solvent?

A

Yes

38
Q

Will a non-polar solute dissolve in a non-polar solvent?

A

Yes

39
Q

Will a polar solute dissolve in a non-polar solvent?

A

No

40
Q

What is the saturation point?

A

Where the maximum solubility is reached

41
Q

What does saturation point depend on?

A

Temperature, pressure (gas) & chemical structure

42
Q

What happens to the freezing, melting & boiling point when adding a solute to water?

A

Decease in freezing & melting point, increase in boiling point

43
Q

What happens if you add salt to ice?

A

Makes it easier to melt

44
Q

What happens to the boiling and freezing point if you add salt to water?

A

Make it harder to freeze & require higher temperature to boil

45
Q

What is evaporation used for?

A

Separate a dissolved solid from a liquid, liquid is lost & solid retained

46
Q

What is distillation used for?

A

Separating 2 liquids

47
Q

How does distillation work?

A

Heating & cooling is used to separate 2 liquids, relies on a difference in boiling point

48
Q

What is filtration used for?

A

Separating solid from a liquid, only work on heterogenous mixtures

49
Q

What is chromatography used for?

A

Separating liquid-liquid, solid-liquid, solid-solid

50
Q

Rough steps of chromatography

A

Mixture is dissolved into a mobile phase (gas or liquid)
Mobile phase flows through the chromatography system
Mixture is separated onto the stationary phase (a piece of paper)

51
Q

What is centrifugation used for?

A

Separate solids from liquids or liquids from liquids, has to be a heterogeneous mixture

52
Q

What is the separation Method of chromatgraphy?

A

Polarity, size, binding affinity, boiling point or charge

53
Q

What is crystallization used for?

A

Separating a solid from a liquid in a homogeneous mixture

54
Q

What is important in order to be able to use crystallization?

A

The solid should have a crystalline structure

55
Q

What principle is crystallization based on?

A

That solubility of a solid in a liquid generally increases with temperature increase & decreases with a temperature decrease

56
Q

Is crystallisation a physical or chemical change?

A

Physical

Chemistry (10 decks)

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