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Chemistry Module 5 > Chapter 1 Rates, equilibrium and pH > Flashcards

Chapter 1 Rates, equilibrium and pH Flashcards

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1
Q

What is the rate equation?

A

k[A]^m [B]^n

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2
Q

What is rate of reaction?

A

The change in concentration of a reactant or a product per unit time.

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3
Q

How do you calculate the overall order?

A

Sum of individual orders

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4
Q

What is meant by order?

A

The order of reaction with respect to a certain chemical shows how changing the concentration of that chemical affects the rate of reaction.

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5
Q

What is zero order?

A
  • Shows rate of reaction doesn’t change with concentration
  • Half life decreases with time
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6
Q

What is first order?

A
  • As concentration halves, the rate of reaction halves
  • Half life is constant
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7
Q

What is second order?

A
  • As concentration halves, rate of reaction goes down by 4 (2^2)
  • Half life increases
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8
Q

What are the units for rate?

A

mol dm^-3 s^-1

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9
Q

What is meant by half life?

A

Time take for the concentration of reactant to fall by half.

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10
Q

What is meant by the rate determining step?

A

Slower step in the reaction

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11
Q

What is the relation between the rate equation and rate determining step?

A

They have the same reactants

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12
Q

What is the Arhenius equation?

A

k=Ae^-Ea/RT
k - rate constant
T - temperature (K)
R - 8.13 JK-1 mol-1
Ea - activation energy

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13
Q

What is the Arhenius equation in the y=mx+c format?

A

lnk = -Ea/RT + lnA

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14
Q

What is a homogenous reaction?

A

All chemicals are in the same states

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15
Q

What is Kc?

A

Equilibrium constant for concentration

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16
Q

What is Kp?

A

Equilibrium constant for pressure

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17
Q

What is the mole fraction?

A

The proportion of a given substance that is present in the reaction mixture

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18
Q

What is partial pressure?

A

The pressure exerted by an individual gas if it occupied the whole vessel on its own

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19
Q

What is the algebraic equation for Kc?

A

Kc = [C]^c [D]^d / [A]^a [B]^b

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20
Q

What is the algebraic equation for Kp?

A

Kp = (PC)^c (PD)^d / (PA)^a (PB)^b

21
Q

How would you calculate the mole fraction of A?

A

moles of A/ total number of moles

22
Q

How do you calculate partial pressure of A?

A

mole fraction of A x total pressure

23
Q

What factors don’t affect the equilibrium constant?

A

Concentration and pressure

24
Q

How does temperature affect the equilibrium constant?

A

If changing temperature causes less product to form, the equilibrium moves to the left and the equilibrium constant decreases.
If changing temperature causes more product to form, the equilibrium moves to the right and the equilibrium constant increases.

25
Q

What is a Bronsted-Lowry acid?

A

A proton donor

26
Q

What is a Bronsted-Lowry base?

A

A proton acceptor

27
Q

What is meant by a dibasic acid?

A

Each molecule can release 2 protons

28
Q

What is meant by a tribasic acid?

A

Each molecule can release 3 protons

29
Q

What is a conjugate acid-base pair?

A

A set of 2 species that transform into each other by gain or loss of a proton

30
Q

What is an alkali?

A

A base that dissolves in water forming OH- ions

31
Q

What is the equation for acid dissociation constant (Ka)?

A

Ka = [H+][A-] / [HA]

32
Q

What does a large Ka value show?

A

It is a stronger acid

33
Q

What does a pKa value represent?

A

similar to pH - lower value=more acidic/ greater dissociation

34
Q

What is the equation for pKa?

A

pKa = -logKa

35
Q

What is the equation for pH?

A

pH = -log[H+(aq)]

36
Q

What is the equation for hydrogen ions concentration?

A

[H+(aq)] = 10^-pH

37
Q

How do you calculate the pH of a strong acid?

A

[HA] = [H+]
pH = -log[H+]

38
Q

How do you calculate the pH of a weak acid?

A

Calculate [H+] using Ka = [H+]^2/[HA]
pH = -log[H+]

([H+]=[A-])

39
Q

How do you calculate the pH of a strong base?

A

[XOH] = [OH-]
Calculate [H+] using Kw = [H+][OH-] = 1x10^-14 (at 25°C)
pH = -log[H+]

40
Q

What are buffers made from?

A

Weak acid and it’s salt or an excess of weak acid and a strong alkali

41
Q

What is a buffer solution?

A

A mixture that minimises pH changes on addition of small amounts of an acid or base.

42
Q

How does a buffer regulate pH?

A

If an acid increases the amount of H+ ions, equilibrium will shift to the left, restoring equilibrium by reacting the ions with the conjugate base, maintaining [H+] and therefore the pH.
If a base increases the amount of OH- ions, equilibrium will shift to the right to restore equilibrium by reacting the ions with the weak acid, maintaining [H+] and therefore the pH.

43
Q

What is the equation for adding OH- ions to a buffered solution?

A

OH- + H+ → H2O
(reacting with weak acid)

44
Q

What is the equation for adding H+ ions to a buffered solution?

A

A- + H+ → HA
(reacting with conjugate base)

45
Q

What is the buffer in the blood? (+equation)

A

Carbonic acid (H2CO3) and its conjugate base (HCO3-)
H2CO3 ⇌ H+ + HCO3-

46
Q

What is Kw?

A

The equilibrium constant for water.

47
Q

What is the equation for Kw?

A

Kw = [H+][OH-] = 1 x 10^-14

48
Q

Is ammonia a strong or weak base?

A

Weak base

49
Q

Give 3 examples of strong acids

A
  • HCl
  • HNO3
  • H2SO4

Chemistry Module 5 (3 decks)

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