# Physical Sciences Grade 12 P2 Western Cape Mock 2025 QP

> Grade 12 Physical Sciences Paper 2 question paper from the Western Cape Mock Exam 2025, 19 pages. Read online or download the free PDF.

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- Updated: 2026-09-27
- Subject: Physical Sciences
- Grade: Grade 12
- Document type: Question paper
- Year: 2025
- Exam period: Western Cape Mock Exam
- Paper: 2
- Curriculum: CAPS
- Pages: 19

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### Page 1

Western Cape
Government

Education

METRO CENTRAL EDUCATION
DISTRICT

GRADE 12
: PHYSICAL SCIENCES: CHEMISTRY (P2) :
: SEPTEMBER 2025
MARKS ; 150
TIME 4 3 hours
DATE 25 SEPTEMBER 2025

This question paper consists of 15 pages and 4 data sheets

### Page 2

Page 2 of 19

INSTRUCTIONS AND INFORMATION

1.

2:

10.

11.

a2.

Write your Name and Surname on the first page of your ANSWER BOOK.

This question paper consists of 9 QUESTIONS. Answer ALL the questions in
the ANSWER BOOK.

Start EACH question on a NEW PAGE of your RULED A4 PAPER. Use BOTH
sides of the page to avoid wasting paper.

Number the answers correctly according to the numbering system used in this
question paper.

Leave ONE line between two sub-questions, for example between QUESTION 2.1
and QUESTION 2.2 or 2.1.1 and 2.1.2

You may use a non-programmable calculator.

You may use appropriate mathematical instruments.

You are advised to use the attached DATA SHEETS.
Show ALL formulae and substitutions in ALL calculations.

Round off your final numerical answers to a minimum of TWO decimal places.
In multi-step calculations, intermediate steps, round of to four decimal places.

Give brief motivations, discussions, et cetera where required.

Write neatly and legibly.

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QUESTION 1: MULTIPLE-CHOICE QUESTIONS

Four options are provided as possible answers to the following questions. Each question
has only ONE correct answer. Choose the answer and write only the letter (A — D) next to
the question number (1.1 — 1.10) on your RULED A4 PAPER, for example 1.11 D.
1.1. Consider the condensed structural formula:
CH3COCH3

Identify the name of the functional group in this formula.

A. Formyl group

B. Carboxyl group

Cc. Ketone

D. Carbonyl group (2)

1.2 | Anorganic compound is incorrectly named as 4,5-dibromo-2-ethylhexane.

The CORRECT IUPAC name for this compound is:

A. 2,3-dibromo-5-ethylhexane

B. 2,3-dibromo-5-methylheptane

Cc. 5,6-dibromo-3-methylheptane

D 5,6-dibromo-3,3-dimethylhexane (2)
1.3 Learners investigate the boiling points of the first five straight chain CARBOXYLIC

ACIDS. Which of the following factors CANNOT be used explain the increase in

boiling points as the number of carbon atoms increases?

A. _ Increase in chain length

B. Increase in surface area

C. Increase in strength of hydrogen bonds

D

Increase in molecular mass (2)

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1.4

1.5

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An alkane reacts with Brz in a laboratory. Which of the following shows the correct
combination of the REACTION CONDITION, the TYPE OF REACTION and the
MAIN PRODUCT of the reaction?

REACTION TYPE OF MAIN
CONDITIONS REACTION PRODUCT
A Conc. NaOH Elimination Haloalkane
|B Suntight Substitution Alcohol
Cc Conc. H2SO« Elimination Alkene
D UV light Substitution Haloalkane
(2)
What is the HEAT OF THE REACTION (AH) and ACTIVATION ENERGY for
the reverse reaction?
ou
2
a
ra)
2
= Reacion coordinate
L
re I Of ) ope ees ee 08 © ares
Vv
HEAT OF REACTION ACTIVATION ENERGY
(AH IN KJ) (KJ)
A 140 60
B -140 20
Cc -140 -140
D 140 160
(2)

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1.6 In an experiment, a 10 g lump of zinc and a 5 g lump of zinc are added to separate
flasks containing the same volume of excess sulphuric acid. The solid line in the
graph shows the volume of gas given off when the 10 g lump of zinc is used.

Which dotted line is obtained when 5 g lump of zinc is used?

‘Time (minutes)
A. Curve A
B. Curve B
Cc. Curve C
D. Curve D (2)
1.7. Asolution of ethanoic acid (acetic acid) is titrated against a standard sodium
hydroxide solution. Which of the following indicators would be the most suitable
for this titration?
INDICATOR pH RANGE OF THE INDICATOR
A Phenolphthalein 8,3 -—10
B Methyl orange 3,1-4,4
Cc Bromothymol blue 6,0-7,6
D Universal indicator Change colour over a wide range of
pH values
(2)

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1.8 The graph below refers to the equation: 2HBr (g) = H2(g) + Br2(g)
Which ONE of the following statements is INCORRECT at time ta?

2HBr(g)

Concentration

H2(g) + Br2(g)

ta Time

The slope of PQ represents the rate at which the concentration
of 2HBr(g) decreases.

The slope of XY represents the rate at which the concentration
of H2(g) and Brz (g) increase.

The rate at which the concentration of 2HBr(g) decreases is not equal
to the rate at which the concentration of H2(g) and Bra(g) increases.

The slopes of PQ and XY are not affected by temperature changes. (2)

1.9 According to the Table of Standard Reduction Potentials, Sn is a stronger reducing

agent than:

A. Ag

B. Zn

Cc. Ni

D. Mn (2)

1.10 During the electrolysis of concentrated sodium chloride solution:

A.

B.

Sodium hydroxide forms at the anode.

Hydrogen forms at the positive electrode.

Sodium forms at the cathode.

Chlorine gas forms at the positive electrode. (2)

[20]

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QUESTION 2 {Start on a NEW page)

The letters A to F in the table below represent six organic compounds:

A | 5-ethy!-2,6-dimethylhept-3-yne CHsCH2CH3
C.] CsH10O D | CsHi20
= :
H Oo H H H
| i | | |
H—- CC — C —~ €C — C —~ C — H
| | | |
H H H H
F | C4HsOH

Use the information in the table (where applicable) to answer the questions that follow.

2.1 Write down the letter(s) representing:

2.1.1. An unsaturated hydrocarbon (1)

2.1.2 A compound that it used as a fuel (1)
2.2 For compound A, write down the:

2.2.1 General formula of the homologous series to which it belongs (1)

2.2.2 Structural formula (3)
2.3. Compound C is a functional isomer of compound E.

Write down the IUPAC name of compound C (2)
2.4 Compound D is a tertiary alcohol whereas compound F is a secondary alcohol.

Write down the:

2.4.1 IUPAC name of compound F (2)

2.4.2 Structural formula of compound D (2)
2.5 Write down the balanced equation using MOLECULAR FORMULAE for the

complete combustion of compound B. (3)

[15]

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QUESTION 3 (Start on a NEW page)

The table below shows the boiling points of some organic compounds.

3.1

3.2

3.3

3.4

3.5

3.6

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ORGANIC COMPOUND BOILING POINT (°C)
A Ethanol 79
B Propan-1-ol 97
c Butan-1-ol 117
D Pentan-1-ol 138
E Pentane X
F Pentanoic acid ¥

Define the term boiling point

(2)

Refer to compounds A to D. When comparing their boiling points, write down:

3.2.1 The independent variable.

3.2.2 One control variable.

(1)
(1)

Fully explain the increase in boiling point from compound A to D by referring to
the TYPE, STRENGTH and ENERGY of the intermolecular forces.

Refer to compounds D and E. Is it fair to compare their boiling point?

Write down YES or NO. Explain the answer.

Which compound, D or E, has a higher boiling point?
Explain the answer by referring to the TYPE, STRENGTH and ENERGY of

the intermolecular forces.

(3)

(2)

(3)

Compound B reacts with another compound to form the product compound Z,
the functional isomer of compound F. Which compound F or Z will have the
higher vapour pressure. Give a reason for the answer.

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(2)
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QUESTION 4 (Start on a NEW page)

In the flow diagram below, a secondary bromoalkane, compound A, is used as a
starting reactant to form different organic compounds under different reaction conditions.
Use the diagram below to answer the questions that follow.

Compound B
(Alcohol)

3
CompoundA Ss
Minor S
Compound C @
x&
Reaction 1
Niajor Compound D

Compound E

CH,CH,CH,CH,

It is given that Reaction 1 and Reaction 2 both use sodium hydroxide (NaOH) as a reagent.
4.1. Write down the structural formula of compound A (2)
4.2 In Reaction 1 concentrated NaOH is used. Write down:
4.2.1. The type of reaction. (1)
4.2.2 The STRUCTURAL FORMULA of compound C. (2)

4.3. In Reaction 2 dilute NaOH is used. Write down the balanced chemical equation
using CONDENSED STRUCTURAL FORMULAE.

No reaction condition is required. (3)
4.4 State TWO reaction conditions for Reaction 3. (2)
4.5 Write down the TYPE of addition reaction represented by Reaction 4. (1)

4.6 Consider Reaction 5. Write down:

4.6.1 ONE reaction condition. (1)
4.6.2 The general formula of the homologous series to which the PRODUCT

belongs. (1)

[13]

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QUESTION 5 (Start on a NEW page)
5.1. The decomposition of hydrogen peroxide is given below:
2H202(t) + 2H2O0(2) + O2(g)  ...... eee AH = - 203 kJ-mott

The energy-profile graph for the decomposition of H2O2 is shown below:

NOT TO SCALE

Chemical potential energy,
Ep (kJ-mol)

Course of reaction

5.1.1 Define the term activated complex. (2)
5.1.2 Calculate the energy released, Y. (2)

5.1.3 Manganese dioxide (MnOz) can be used as a catalyst in the decomposition
of hydrogen peroxide.
Redraw the above graph and on the same system of axes draw the curve
that will be obtained for the catalysed reaction and label the catalysed
activated complex as C. (2)

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5.2 Four experiments, P, Q, R and §S, are carried out to investigate factors that affect
the rate of decomposition of hydrogen peroxide, H2O2(£).

Identical samples of hydrogen peroxide are used in each experiment.

The conditions used in each experiment are summarised in the table below.

EXPERIMENT | TEMPERATURE (°C) CONDITIONS
P 20 Without catalyst
Q 20 With MnOz catalyst
R 40 Without catalyst
Ss 40 With MnOz catalyst

5.2.1 Define the term reaction rate.

5.2.2 Compare EXPERIMENTS P and R.

Which experiment P or R, will have the higher reaction rate?
Use the collision theory to explain the answer.

5.3. The decomposition of hydrogen peroxide is given below:

2H,0.(t) >

(2)

(3)

2HO(8) + O29) veeereevee AH = - 203 kJ-mot"

During EXPERIMENT §, the following results for the decomposition of hydrogen
peroxide are obtained:

TIME (s) H202 CONCENTRATION (mol-dm*)
0 0,0100
100 0,008
200 X
300 0,0053
400 0,0043

5.3.1. The rate of reaction during the first 200 s is 1,73 x 10° mol-dm*- s*.

Calculate the concentration, X, of H2O2.

(4)

5.3.2 Calculate the volume of oxygen produced within the first 300 s if 25 cm®
of hydrogen peroxide decomposes in this time interval.

Take the molar gas volume as 25,7 dm? -mol"

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(6)
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QUESTION 6 (Start on a NEW page)

The hypothetical reaction represented by the balanced equation below reaches chemical
equilibrium in a closed container at temperature T °C.

Qz.(g) + RS3(g) = 2QS(g) + RS(s)
6.1 Define the term chemical equilibrium. (2)

6.2 Initially 0,6 moles of Q2(g), 0,6 moles of RSa(g), 0,4 moles of QS(g) and
0,4 moles of RS(s) were mixed and sealed in a 500 cm? flask.

If the equilibrium constant (Kc) for this reaction at temperature T °C is 0,04,

Calculate to THREE decimal places, the CHANGE IN THE NUMBER OF

MOLES of Qz. (7)
The temperature is now increased causing the amount of Q2 in the container to decrease.
6.3. What is the sign of AH for the forward reaction?

Write down POSITIVE or NEGATIVE. Fully explain the answer. (3)
Further changes are made to the above equilibrium mixture.

The graph below shows how reaction rate changes with time.

Forward reaction:

2 — Reverse reaction: -— — —
1

Bs}

a

o

w

) 10 20 30 t(s)
6.4 Write down the disturbance responsible for the change observed at t = 10 s. (1)

6.5 Fully explain the change in reaction rate of both the forward and the reverse
reactions from t= 10 stot = 20s. (3)

6.6 A suitable catalyst is now added to the reaction mixture at t = 30 s.
Redraw the above graph from 20 s to 30 s. On the same system of axes draw
the change(s) in the graph, if any, from 30 s onwards. (2)

[18]

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QUESTION 7 (Start on a NEW page.)

7.1

7.2

7.3

Consider the following acid-base reactions, X and Y.
X: H2SO4 + Ho = HSO4 + H30*

Y: HSOs + HO = SO, + H30*

7.1.1 Define the term acid according to the Arrhenius theory. (2)
7.1.2 Write down the NAME or FORMULAE of the substance that acts as an
ampholyte. (1)
7.1.3. Write down the FORMULAE of the conjugate acid in reaction X. (1)
7.1.4 Calculate the pH of a 0,3 mol:dm* sulphuric acid solution. (3)

A solution is made by dissolving NazCO:(s) in water.

7.2.1 Will the solution of NazCOz have a pH EQUAL to 7, LESS THAN 7 or
GREATER THAN 7? (1)

7.2.2 Write down a balanced chemical equation to explain the answer to
QUESTION 7.2.1 (2)

An IMPURE sample of sodium carbonate (NazCOa(s)) with a mass of 5 g is added
to a 100 cm? volume of sulphuric acid of a pH of 0,2. After the reaction is complete,
the EXCESS H2S0Oz, is titrated with 0,1 mol-dm® NaOH of volume 50 cm?.

The following reactions take piace during the above process:

Reaction 1: H2SOa(aq) + NazCO3(s) —» NazSOa(aq) + CO2(g) + H2O()

Reaction 2: H2SO4(aq) + 2NaQH(s) — NazSOa(aq) + H2O(£)

7.3.1 Calculate the initial concentration of the sulphuric acid solution. (3)
7.3.2 Calculate the percentage purity of the NazCOs sample (7)
[20]

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QUESTION 8 (Start on a NEW page.)
The following reaction takes place in a galvanic cell under standard conditions.
Mg(s) + X**(aq) + Mg?*(aq) + X(s)
8.1. Write down the energy conversion that takes place in this cell. (1)
8.2 Write down the half reaction taking place at the ANODE. (2)

8.3 Explain in terms of CHANGES IN OXIDATION NUMBERS, why X°**(aq) is the
oxidising agent. (1)

The Mg half-cell is replaced with a chlorine half-cell as shown in the diagram below.
The electrochemical cell below also functions under standard conditions.

chlorine gas
platinum —
1 mol-dm? Ct(aq) —4
Half-cell A Half-cell B
8.4 Give areason why platinum is used as the electrode in half-cell A. (1)

8.5 Besides concentration, state TWO other standard conditions for the above
electrochemical cell. (2)

8.6 Write down the cell notation for the above electrochemical cell. (3)

8.7 The initial emf of this cell is 2,10 V. Using a suitable calculation, determine the
NAME or FORMULA of metal X. (5)

8.8 What will be the effect on the cell potential when a small amount of silver nitrate
solution, AgNOs (aq), is added to half-cell A? Choose from INCREASES,
DECREASES or REMAINS THE SAME. Explain the answer.

(HINT: Silver chloride is an insoluble salt.) (3)

[18]

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QUESTION 9 (Start on a NEW page.)

The diagram below shows an electrolytic cell that is used to electroplate an iron rod with
copper. Solution X is made up of an UNKNOWN nitrate.

Power
source
Iron rod —j iH A
+—_+— Solution X
Solution X is an electrolyte.
9.1 Explain the term electrolyte. (2)
9.2 Write down the FORMULA of solution X. (1)
9.3. Which electrode (A or iron rod) is the cathode?
Give a reason for the answer. (2)

9.4 Write down the half reaction that takes place at electrode A. (2)

Electrode A is now replaced by a silver rod without making any other changes to the
cell. After a while, TWO metallic ions are found to be present in the solution.

9.5 Name the TWO metallic ions present in the solution. (2)

9.6 Refer to the relative strength of oxidising agents to explain which ONE of the
two ions will preferably be involved in the plating process. (2)

[11]

TOTAL 150 MARKS

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DATA FOR PHYSICAL SCIENCES GRADE 12
PAPER 2 (CHEMISTRY)

GEGEWENS VIR FISIESE WETENSKAPPE GRAAD 12
VRAESTEL 2 (CHEMIE)

TABLE 1: PHYSICAL CONSTANTS/TABEL 1: FISIESE KONSTANTES

NAME/NAAM SYMBOL/SIMBOOL VALUE/WAARDE
Standard pressure 0 5
Standaarddruk P 1,013 x 10° Pa

Molar gas volume at STP

3. -1
Moléregasvolume by STD Vm 22,4 dm*-mot
Standard temperature ‘i
Standaardtemperatuur T 273 K
Charge on electron _ 49
Lading op elektron & 18 WIE
Avogadro's constant Na 6,02 x 1023 mol"

Avogadro-konstante

TABLE 2: FORMULAE/TABEL 2: FORMULES

m N
n=— n=—
M Na
é-". orlofe = ne
V MV Vin
C,V n
Sa = 3 pH = -log[H30*]
CLV_ ny

Kw = [H30*][OH] = 1 x 10-4 at/by 298 K

8 8 8 8 8 6
Econ = a ~ E088 1B Sei = EKatode ~ Esse
or/of

8 8 8 C) 8 8
Een = Erauenen ~ Eo dation/ Eger = Erecuaie: — Eoxcaae
or/of
E°, =E° - Ee /E°, = ES — Ee

cell ~ “oxidisingagent reducingagent sel ~ “oksideermiddel reduseermiddel

Q n= a where n is the number of electrons/

[= At Ge waar n die aantal elektrone is

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TABLE 3: THE PERIODIC TABLE OF ELEMENTS

1 2 3 4 5 6 ri 8 9 10 1 12 13 14 15 16 17 18
) ) quveraraus (ly) (vy) (Vy) vy)
4 KEY/SLEUTEL a tat 2
es foomgetai
x H as He
1 a 4
3 r Electronegativity | oy 4 Symbol 5 6 7 8 9 10
= Li |? Be Elektronegatiwitett | ~ 63.5 Simbool a a Cis N ls O |S Ne
7 9 + 11 12 14 16 19 20
11 12 13 14 15 16 17 18
roximate relative atomic mass ale
2 Na | Mg *pP fae? sils P&S |$ce| Ar
23 24 Benaderde relatiewe atoommassa 27 28 31 32 35,5 40
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
3 K [2 Cal? Se [2 Ti|2 V [2 Cr/2Mnj/e Fe |= Co|2 Ni |? Cu|2 Zn|2 Ga|2 Ge|& As |x Se |x Br| Kr
39 40 45 48 51 52 55 56 59 59 63,5 65 70 (é) 75 79 80 84
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54
& Rb|2 Sr|2 Y |S Zr} Nb\= Mol? Tels Ruis Rh|w Pd|? Ag |= Cd/= In |2 Sn|2 Sb a Te | Xe
86 88 89 91 92 96 101; 103; 106) 108) 112} 115| 119| 122| 128| 127/ 131
55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
3 Cs|$ Ba| La\? Hf} Ta} W/ Re} Os| Ir| Pt| Au) Hg/= Te|2Pb\2 Bi|s Po/s At} Rn
133 137 139 | 179} 181 184; 186; 190} 192] 195| 197| 201| 204| 207) 209
87 88 89
> Fr |S Ra Ac
= S 226 58 59 60 61 62 63 64 65 66 67 68 69 70 11
Ce Pr Nd | Pm | Sm | Eu | Gd Tb Dy Ho Er | Tm | Yb Lu
140 | 141 | 144 150 | 152 | 157 | 159 | 163 | 165 | 167 | 169 | 173 | 175
90 91 92 93 94 95 96 97 98 99 100 | 101 | 102 | 103
Th Pa U Np Pu | Am | Cm | Bk Cf Es Fm | Md | No Lr
232 238

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Increasing oxidising ability/ Toenemende oksiderende vermoé

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TABLE 4A: STANDARD REDUCTION POTENTIALS

Half-reactions/Halfreaksies E 8 (Vv)
Fo(g)+2e = 2F + 2,87
Co +e = Cor + 1,81
H202+ 2H*+2e = 2H20 41,77
MnO, +8H*+5e = Mn%+4H2O | +1,51
Ch(g)+2e = 2Ch + 1,36
CrOe +14H++6e = 2Cr*+7H20 | +1,33
O2(g)+4H*+4e° = 2H20 + 1,23
MnOz+ 4H* + 2e == Mn?+ + 2H20 + 1,23
Pt*+2e = Pt + 1,20
Bro(t)+2e- = 2Br +1,07
NO, +4H*+3e = NO(g)+2H20 | +0,96
Hg?t+2e- = Hg(t) + 0,85
Agt +e Ag + 0,80
NO, +2H'+e = NO2(g)+H20 | +0,80
Fe++e = Fer +0,77
O2(g) + 2H*+2e = H2O2 + 0,68
@e+2e = ab + 0,54
Cur +e Cu + 0,52
SO2+4H*+4e = S$+2H20 + 0,45
2H20+O2+4e = 4OH + 0,40
Cur+ + 2e Cu + 0,34
SO; +4H'+2e = SOx(g)+2H20] +0,17
Cut+e = Cur +0,16
Sn4++2e = Snét +0,15
S+2Ht+2e = HeS(g) +0,14
2H*++2e- = Ha2(g) 0,00
Fe3++3e = Fe — 0,06
Pb2*+2e = Pb — 0,13
Sn2*+2e = Sn —0,14
Ni2++2e = Ni —0,27
Co2++2e = Co -0,28
Cd2++2e = Cd —0,40
Cre++e = Crt — 0,41
Fet*+2e° = Fe — 0,44
Cr++3e = Cr —0,74
Zn?*+2e = Zn - 0,76
2H20 +2e- = Ha(g)+20H- | -0,83
Cre++2e = Cr -0,91
Mn2*+2e = Mn —1,18
AG++3e = At — 1,66
Mg2*+2e = Mg — 2,36
Nat+e = Na -2,71
Cat*+2e = Ca — 2,87
Sr++2e = Sr — 2,89
Bat++2e = Ba — 2,90
Cst+e = Cs - 2,92
Kt+te = K — 2,93
Ltée = Li — 3,05

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Increasing reducing ability/ Toenemende reduserende vermoé

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bility/ Toenemende oksiderende vermoé

ising al

id

Increasing Oxi

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TABLE 4B: STANDARD REDUCTION POTENTIALS

Half-reactions/Halfreaksies £9 (V)
litte = Li -3,05
Kt+e = K -— 2,93
Cst+e = Cs — 2,92
Ba?* + 2e Ba — 2,90
Srt+2e = Sr — 2,89
Ca2*+2e = Ca —2,87
Na*+e = Na -271
Mg?++2e- = Mg — 2,36
AG++3e = AL — 1,66
Mn?* + 2e- Mn —1,18
Cr++2e = Cr —0,91
2H20 + 2e- = H2(g) + 20H” — 0,83
Zn2++2e = Zn —0,76
Cr+ + 3e- Cr — 0,74
Fee + 2e- Fe — 0,44
Cette = Crt -0,41
Cd*+2e = Cd —0,40
Co +2e = Co — 0,28
Ni2++2e = Ni -0,27
Sn%+2e = Sn — 0,14
Pb4++2e° = Pb — 0,13
Fes++3e = Fe — 0,06
2H*++2e- = H2(g) 0,00
S+2H*+2e = HeS(g) + 0,14
Sn*+2e = Sn +0,15
Cu2t+e = Cut + 0,16
S07 +4H*+2e = SOd(g)+2H20|} +0,17
Cu2++2e = Cu + 0,34
2H20+O2+4e = 40H + 0,40
SO2+4H++4e = S+2H20 + 0,45
Cut+e = Cu + 0,52
la+2e = 2 + 0,54
O2(g)+2H*+2e = H2O2 + 0,68
Fe**+e- = Fe2+ +0,77
NO; +2H*+e = NOa(g)+H20 | +0,80
Agi+e = Ag + 0,80
Hg?++2e- = Hg(t) + 0,85
NO 3 +4H*+3e- = NO(g)+2H20 | +0,96
Br(t)+2e = 2Br + 1,07
Pt++2e = Pt + 1,20
MnO2t 4H* + 2e° = = Mn?* + 2H20 + 1,23
O2(g)+4H++4e- == 2H20 + 1,23
Cros +14H++6e = 2Cr*+7H2O | +1,33
Ch(g)+2e = 2Ch + 1,36
MnO 4 +8H*+5e = Mn? +4H20 +1,51
H2O2+2H*+2e = 2H20 44,77
Co3*+e = Cor + 1,81
Fo(g)+2e- =F + 2,87

ity/ Toenemende reduserende vermoé

Increasing reducing abi

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