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chemistry > U1 : Topic 5 Equilibrium > Flashcards

U1 : Topic 5 Equilibrium Flashcards

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1
Q

When is a chemical reaction at equilibrium?

A

When the rate of the forward reaction is equal to the rate of the reverse reaction.

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2
Q

When a reaction mixture has reached equilibrium the composition of the reactants and products ….

A

Remain constant.

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3
Q

Increasing concentration of reactant effect?

A

Increase rate of forward reaction equilibrium moves to the right.

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4
Q

Increase concentration of product effect?

A

Increase the rate of reverse reaction so equilibrium moves to the left.

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5
Q

Increase temperature effect?

A

Favours endothermic reaction equilibrium moves in direction of endothermic.

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6
Q

Increase pressure effect?

A

Favours a decrease in pressure equilibrium moves to side with fewest moles of gas.

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7
Q

Use of catalyst effect?

A

No effect (reaches equilibrium. faster)

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8
Q

What is the constant K?

A

Ratio between the reactants and products.

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9
Q

[A], [B],[C],[D] are what?

A

Concentrations at equilibrium.
Can be expressed as number of moles or pressure as well as concentration.

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10
Q

a, b, c, and d are what?

A

The stoichiometric coefficients in the balanced reaction equation. The numbers in front of the formula

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11
Q

The concentrations of pure solids and pure liquids at equilibrium are taken as constant and given value of?

A

1

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12
Q

The equilibrium lies to the left hand side what is the value of K?

A

Less than 1.

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13
Q

If the value of K is 1 what is the position of equilibrium?

A

50% of each

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14
Q

Position of equilibrium is R.H.S what is the value of K?

A

Greater than 1

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15
Q

what factors don’t affect K?

A

Concentration, pressure, addition of catalyst.

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16
Q

When the concentration of a reactant or product is altered what happens to equilibrium?

A

It will adjust to counteract this change. Doing this will change the concentration of other reactants and products but ratio K will remain constant.

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17
Q

If you alter the pressure of the system the equilibrium will adjust the concentrations of?

A

Reactants and products counteracting the pressure change keeping K constant.

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18
Q

How does the addition of a catalyst affect K?

A

No affect to quantities of reactants or products. Reaches equilibrium faster.

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19
Q

The value of K is affected by what?

A

Temperature

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20
Q

Increasing Temperature does what to K in endothermic?

A

Favours endothermic reaction, so equilibrium shifts to the right increasing concentration of products, k increases and so does yield of product.

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21
Q

Exothermic reaction to temperature increase what happens to K?

A

Equilibrium shifts to left increasing concentration of reactants and k decreases yield of products also decreases.

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22
Q

According to Brønsted-Lowry what is the definition of an acid?

A

Proton donor.

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23
Q

According to Brønsted-Lowry what is the definition of a base?

A

Proton acceptor

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24
Q

Water is amphoteric what does this mean?

A

Can act as both an acid and base.

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25
Q

What are examples of strong acids?

A

Hydrochloric acid, sulfuric acid and nitric acid.

26
Q

Strong acids completely what?

A

Dissociate into ions in aqueous solutions.

27
Q

Examples of weak acids?

A

Ethanoic acid, carbonic acid and sulfurous acid.

28
Q

Weak acids only partially what?

A

dissociate into ions in aqueous solution.

29
Q

When carbon dioxide and other non-metal oxides dissolve in water they produce?

A

Acidic solutions

30
Q

What does Equimolar mean?

A

Solutions that contain the same number of moles.

31
Q

A strong acid has a ……. pH than a weak acid.

A

Lower.

32
Q

A strong acid has a …… conductivity than a weak acid.

A

Higher

33
Q

A Strong acid has a ………. rate of reaction with Mg than a weak acid.

A

faster

34
Q

Compared to a weak acid a strong acid has an equal what?

A

Stoichiometry.

35
Q

The more hydrogen ions present the lower the ….. , the higher the …… and the faster the …….

A

pH
Conductivity
Rate of reaction

36
Q

Strong acid concentration will be equal to concentration of?

A

H+ ions.

37
Q

Since a weak acid only partially dissociates the concentration of h+ ions will be?

A

Much lower than the acid.

38
Q

Ka is a measure of what?

A

Strength of acid.

39
Q

In strong acids Ka has what?

A

No meaning

40
Q

The smaller the value of Ka the …… the acid.

A

Weaker.

41
Q

when an acid is diluted the pH increases towards?

A

7

42
Q

Examples of strong bases?

A

metal hydroxides (calcium hydroxide, sodium hydroxide)

43
Q

Strong based completely…… in aqueous solutions.

A

dissociate into ions in aqueous solutions.

44
Q

what are examples of weak bases?

A

Ammonia and amines.

45
Q

Weak bases only what in aqueous solutions?

A

Partially dissociate into ions.

46
Q

Strong bases will have ……. pH, …….. conductivity and …….. rate of reaction than weak bases.

A

Higher
Higher
Faster

47
Q

When an alkali is diluted the pH does what?

A

Decreases towards 7.

48
Q

To calculate the pH of strong alkali you need to do what first?

A

Work out concentration of hydrations using Kw.

49
Q

What is formed during a neutralisation reaction?

A

Salt

50
Q

A strong acid and a strong base produce a salt with what pH?

A

Neutral

51
Q

A strong acid and a weak base produce a salt with what pH?

A

less than 7 (acidic)

52
Q

A weak acid and a strong base produce a salt with what pH?

A

greater than 7 (alkaline)

53
Q

Using appropriate equilibrium the change of concentrations of what can be explained?

A

H3O+ and OH- ions of salt solutions.

54
Q

What is a buffer solution?

A

One which the pH remains approximately constant when small volumes of acid, base or water are added.

55
Q

A buffer can be … or ….

A

Acidic or basic.

56
Q

What is an acidic buffer?

A

Solution of weak acid and a salt of weak acid.

57
Q

How does an acid buffer work?

A

The weak acid Provides hydrogen ions when they are removed by the addition of a small amount of base. The salt provides conjugate base which can absorb excess hydrogen ions produced by addition of small amount of acid.

58
Q

What is a basic buffer?

A

Consists of solution of weak base and one of its salts.

59
Q

How does a basic buffer work?

A

The weak base removes excess hydrogen ions and the conjugate acid provided by the salt supplies hydrogen ions when these are removed.

60
Q

What are indicators used for?

A

To show the end point of a titration.

61
Q

What are indicators?

A

Weak acids.

62
Q

Colour of the indicator must be distinctly different from….

A

The conjugate base.

chemistry (7 decks)

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