Alva Academy
Standard Grade Chemistry
Topics 8-15
Homework
Contents
Topic 8 Homework 1 ………… Pages 2, 3
Topic 8 Homework 2 ………… Page 4
Topic 8 Homework 3 ………… Page 5
Topic 9 Homework 1 ………… Pages 6, 7
Topic 9 Homework 2 ………… Page 8
Topic 10 Homework 1 ………… Pages 9, 10, 11
Topic 10 Homework 2 ………… Pages12, 13
Topic 11 Homework 1 ………… Pages 14, 15
Topic 11 Homework 2 ………… Pages 16, 17
Topic 12 Homework 1 ………… Page 18
Topic 12 Homework 2 ………… Page 19
Topic 13 Homework 1 ………… Page 20
Topic 13 Homework 2 ………… Pages 21, 22
Topic 14 Homework 1 ………… Pages 23, 24
Topic 14 Homework 2 ………… Pages 25, 26
Topic 14 Homework 3 ………… Page 27
Topic 15 Homework 1 ………… Page 28
Topic 15 Homework 2 ………… Pages 29, 30, 31
SG Chem Topics 8 to 15 Page 1 Homework
Topic 8 – Homework 1
General Level
1. Using the apparatus below, a pupil electrolysed three
different acid solutions.
hydrogen
acid solution
carbon electrodes
electrode A
battery
It was noted that a gas was given off at electrode A in all
cases. The pupil suspects that the gas is hydrogen.
a. What test would show that the gas is hydrogen? (2)
b. Is A the positive or the negative electrode? (1)
c. Explain your answer to „b‟. (1)
2. X is a solution of an acid, Y is a solution of an alkali.
Below are six statements which may apply to the
solutions.
A: It contains more H+(aq) ions than pure water.
B: It contains more OH-(aq) ions than pure water.
C: It has a pH less than 7.
D: It has a pH equal to 7.
E: It contains ions.
F: It has a pH more than 7.
a. Which statement is correct for both X and Y? (1)
b. Which two statements are correct for X
but not for Y? (2)
SG Chem Topics 8 to 15 Page 2 Homework
Topic 8 – Homework 1 continued
General Level
3. Look at the oxides below and write the letter of the
category that describes them best.
A: Dissolves in water to give a pH less than 7.
B: Dissolves in water to give a pH more than 7.
C: Have no effect on the pH of water.
a. sulphur dioxide d. copper (II) oxide
b. sodium oxide e. iron (III) oxide
c. carbon dioxide f. barium hydroxide (6)
Credit Level
4. Pure water is added to a solution with a pH 12.
a. Which two ions are present in pure water?
b. Which contains more hydroxide ions, the solution or
pure water?
c. What happens to the concentration of hydroxide ions
in the solution as water is added? (4)
SG Chem Topics 8 to 15 Page 3 Homework
Topic 8 – Homework 2
General Level
1. Calculate the formula mass for the following substances.
a. CH4 c. carbon dioxide
b. CaCO3 d. potassium carbonate (4)
2. Calculate the mass of one mole of the following
substances.
a. MgO c. calcium oxide
b. K2O3 d. potassium hydroxide (4)
Credit Level
3. Write the formula then calculate the mass of each of the
following substances.
a. 2 moles of sodium chloride
b. 0.25 moles of magnesium nitrate
c. 0.2 moles of sodium hydrogen sulphate (6)
4. Calculate the number of moles in each of the following
substances.
a. 36g of carbon
b. 5.6g of carbon monoxide
c. 8.2g of calcium nitrate (6)
SG Chem Topics 8 to 15 Page 4 Homework
Topic 8 – Homework 3
Credit Level
1. Calculate the number of moles of potassium hydroxide
which must be dissolved to make each of the following
solutions.
a. 200cm3 of 0.5 mol/l
b. 2 litres of 0.25 mol/l (2)
2. Calculate the number of grams of substance which must
be dissolved to make each of the following solutions.
a. 50cm3 of 2 mol/l sodium hydroxide
b. 25cm3 of 0.2 mol/l lithium nitrate (6)
3. Calculate the concentration of each of the following
solutions.
a. 8g of sodium hydroxide in 250cm3 of solution
b. 4g of copper (II) sulphate in 100cm3 of solution (4)
SG Chem Topics 8 to 15 Page 5 Homework
Topic 9 – Homework 1
General Level
1. a. Explain what is meant by a neutralisation
reaction (2)
b. Name a substance found around the house that
could be used to neutralise spilt battery acid. (1)
c. What will happen to the pH of the acid as it is
neutralised? (1)
d. Explain why gardeners add lime to soil which is too
acidic. (2)
2. Name the products which would be formed in the
reaction between each of the following solutions.
a. potassium hydroxide and nitric acid (1)
b. sodium hydroxide and sulphuric acid (1)
3. During manned flights in space rockets, carbon dioxide
builds up in the air inside the cabin.
a. Explain why the rockets also carry a supply of lithium
hydroxide. (2)
b. What will happen to the pH of the lithium hydroxide
solution during the flight? (1)
4. a. Which gas is produced when a metal carbonate
reacts with a dilute acid? (1)
b. Describe the test for this gas. (1)
5. a. Which gas is produced when a metal reacts with
dilute hydrochloric acid? (1)
b. Describe the test for this gas. (1)
6. Name all the products for each of the following reactions.
a. calcium and hydrochloric acid (1)
b. magnesium and sulphuric acid (1)
SG Chem Topics 8 to 15 Page 6 Homework
Topic 9 – Homework 1 continued
Credit Level
7. Look at the list of substance below.
ammonium chloride copper (II) oxide
potassium sulphate sodium oxide
lithium nitrate barium oxide
zinc oxide
Put these in a table with the headings alkalis, bases and
salts. (7)
SG Chem Topics 8 to 15 Page 7 Homework
Topic 9 – Homework 2
Credit Level
1. Write balanced chemical equations for each of the
following reactions.
a. sodium hydroxide solution and hydrochloric acid. (2)
b. magnesium oxide and nitric acid. (2)
c. potassium carbonate solution and hydrochloric
acid. (2)
d. aluminium and hydrochloric acid (2)
e. copper (II) sulphate solution and sodium hydroxide
solution. (2)
2. a. What volume of hydrochloric acid (concentration 0.1
mol/l) is required to neutralise 50cm3 of sodium
hydroxide solution (concentration 0.2 mol/l)? (2)
b. What is the concentration of sulphuric acid if 50cm3
are neutralised by 25cm3 of potassium hydroxide
solution (concentration 1mol/l)? (2)
c. What volume of nitric acid (concentration 2mol/l) is
required to neutralise 20cm3 of sodium hydroxide
solution (concentration 0.5mol/l)? (2)
d. What is the concentration of hydrochloric acid if
12.6cm3 neutralises 20cm3 of potassium hydroxide
solution (concentration 0.1mol/l)? (2)
e. What is the concentration of sulphuric acid if 17.3cm3
neutralises 25cm3 of sodium hydroxide solution
(concentration 0.5mol/l)? (2)
SG Chem Topics 8 to 15 Page 8 Homework
Topic 10 Homework 1
General Level
1. One of the most widely used batteries is known as the dry
cell. This is used in portable radios, torches and toys.
a. Explain why the dry cell eventually has to be re-
placed. (1)
b. What is the purpose of the ammonium chloride paste
in the dry cell? (1)
c. Explain why the ammonium chloride is in the form of
a paste and not completely “dry”. (2)
d. State one advantage of a nickel-cadmium battery
compared to a dry cell. (1)
e. In a house it is cheaper to run the radio from the
mains or the batteries? (1)
2.
Electron flow
V
A C
E
B D
a. Using magnesium, copper, magnesium sulphate
solution and copper sulphate solution, state what A,
B, C and D must be to give a flow of electrons in the
direction shown. (2)
b. i. What is E on the diagram known as? (1)
ii. Why is it necessary? (1)
iii. Why is sodium chloride solution suitable to be
used in E, but sugar solution not? (2)
SG Chem Topics 8 to 15 Page 9 Homework
Topic 10 – Homework 1 continued
General Level
3. Using the apparatus below, the following results were
obtained.
a. What name is given to this kind of series of metals
arranged from voltmeter readings? (1)
V Filter paper
soaked in sodium
chloride solution
Test metal copper
Test metal Voltmeter reading (volts)
lithium 2.9
Sodium 2.4
Magnesium 1.6
Iron 0.5
Tin 0.4
Copper 0.0
silver -0.4
b. Why doesn‟t magnesium ribbon react with sodium
sulphate solution? (1)
c. When magnesium ribbon is added to copper
sulphate solution, the ribbon starts to break up at the
surface, a brown solid forms, and the solution
eventually becomes colourless. Explain these three
observations. (3)
d. Suppose the copper block was replaced by a block
of tin. What would the reading on the voltmeter be if
the test metal was iron? (1)
e. Which metal could be used as the test metal to give
a voltmeter reading of approximately 1.2 volts? (1)
SG Chem Topics 8 to 15 Page 10 Homework
Topic 10 – Homework 1 continued
Credit Level
4.
V
Carbon Carbon
electrode A electrode B
Potassium Iron(III) chloride
iodide solution solution
Cotton wool plug
The reaction occurring at electrode B is:
Fe3+(aq) + e- ───> Fe2+(aq)
a. Name the type of reaction occurring at electrode B
(1)
b. In which direction do the electrons flow through the
meter? (1)
c. What product is formed from iodide ions at electrode
A? (1)
SG Chem Topics 8 to 15 Page 11 Homework
Topic 10 – Homework 2
Credit Level
1. Decide which of the following reactions involve:
O: oxidation R: reduction
(You may find it helpful to use the data booklet.)
a. Zn2+(aq) + 2e- ───> Zn(s)
b. Ag(s) ───> Ag+(aq) + e-
c. Br2(l) + 2e- ───> 2Br-(aq)
d. SO32-(aq) + H2O ───> SO42-(aq) + 2H+ + 2e-
e. nickel (III) ───> nickel (II)
f. copper atoms ───> copper ions (6)
2. This question refers to the addition of a metal to a
solution containing ions. In each case decide whether
Yes: a reaction will take place.
No: a reaction will NOT take place.
a. copper added to silver nitrate solution (1)
b. magnesium added to sodium sulphate solution (1)
c. iron added to dilute hydrochloric acid (1)
d. copper added to dilute sulphuric acid solution (1)
e. iron added to copper(II) nitrate solution (1)
3. When copper metal is added to a solution of silver(I)
nitrate a displacement reaction occurs forming silver
metal and copper(II) nitrate.
a. Write a balanced equation for the reaction. (2)
b. How many moles of silver are displaced by 1 mole of
copper? (1)
c. What mass of silver will be displaced by 3.2g of
copper? (2)
SG Chem Topics 8 to 15 Page 12 Homework
Topic 10 – Homework 2 continued
Credit Level
4. a. C + O2 ───> CO2
What weight of carbon dioxide is formed when 6g of
carbon is burned completely? (2)
b. 2 Mg + O2 ───> 2 MgO
What weight of magnesium oxide is produced when 24g
of magnesium burns? (2)
c. 2 H2 + O2 ───> 2 H2O
What weight of hydrogen is needed to give 9g of
water? (2)
5. A compound Z is found to contain 54.5% carbon, 9.1%
hydrogen and 36.4% oxygen and have a formula mass of
88amu.
a. Calculate the empirical formula of Z. (4)
b. What is the molecular formula of Z? (1)
SG Chem Topics 8 to 15 Page 13 Homework
Topic 11 – Homework 1
General Level
1. Each of the following experiments were set up to
investigate the rate of four metals, W, X, Y and Z, with
dilute hydrochloric acid.
W X Y Z
a. Place the four metals in order of reactivity. Start with the
most reactive. (1)
b. State three factors that must be kept the same for the
comparison to be a fair one. (3)
c. Which gas is produced in the reaction of a metal with
dilute hydrochloric acid? (1)
d. Write a word equation for the reaction of magnesium with
dilute hydrochloric acid. (1)
e. Write an equation for the reaction using symbols and
formulae. (1)
SG Chem Topics 8 to 15 Page 14 Homework
Topic 11 – Homework 1 continued
General Level
2. The results of experiments with four metals W, X, Y, Z
and their compounds are summarised in the table below.
Metal Column 1 Column 2 Column 3
Reaction of metal Action of heat on Reaction of metal
with dilute acid metal oxide with cold water
W hydrogen evolved no reaction hydrogen formed
X no reaction no reaction no reaction
Y hydrogen evolved no reaction very slow reaction
Z no reaction metal formed no reaction
a. State what information about the order of reactivity
of the metals can be obtained from:
i. Column 1 alone (1)
ii. Column 2 alone (1)
b. Now use ALL the information to put the metals into
an order of reactivity placing the most active first. (1)
c. Suggest a name for each metal W, X, Y and Z. (1)
3. An unknown metal was found to be more reactive than
sodium. Which of the following predictions about the
metal is likely to be correct? (1)
A. It will react readily with oxygen in the air.
B. It should be stored under water.
C. Its compounds will be unstable.
D. It will be obtained from its oxide by heating
with carbon.
SG Chem Topics 8 to 15 Page 15 Homework
Topic 11 – Homework 2
General Level
1. Name one metal which can be extracted by each of the
methods below.
a. By heating alone.
b. By heating with carbon, but not by heating alone.
c. By using electricity but not by heating with carbon. (3)
2. Iron is produced from its ore using a process called
smelting. The chemical reactions take place in a huge
tower.
a. What name is given to the tower? (1)
b. The following reactions take place in the tower. Write
a word equation for each.
i. The burning of coke. (1)
ii. The production of carbon monoxide gas. (1)
iii. The formation of iron from its ore. (1)
Credit Level
3. A pupil was asked to investigate three metal oxides LO,
M2O, and NO. On heating strongly LO broke down into a
metal L and oxygen. The other two oxides did not break
down.
a. From this evidence what can be deduced about the
reactivity of metal L. (1)
b. How could you test M2O and NO in order to find
out which was the more reactive of the metals M
and N? (1)
4. Calculate the simplest (empirical) formula for the
following compounds from the percentage composition
by mass.
a. 25% magnesium, 75% chlorine
b. 33% calcium, 27% sulphur, 40% oxygen (4)
SG Chem Topics 8 to 15 Page 16 Homework
Topic 11 – Homework 2 continued
Credit Level
5. A container when empty had a mass of 60g. An oxide of
lead was added and the mass of the container plus the
oxide was 120g. Carbon monoxide gas was then passed
over the heated oxide. During the reaction lead oxide
was reduced to lead. At the end of the reaction the mass
of the container plus the lead metal was 112g.
What is the simplest formula for the oxide? (2)
SG Chem Topics 8 to 15 Page 17 Homework
Topic 12 – Homework 1
General Level
1. a. Apart from iron, what two substances are necessary
for rusting to occur? (2)
b. When iron rusts, what happens to the iron atoms? (1)
2. a. How does ferroxyl indicator help to compare the rates
of corrosion? (1)
b. Explain why salt in the water speeds up the rate of
corrosion whereas glucose does not. (1)
Credit Level
3. Corrosion involves atoms at the surface of a metal losing
electrons and changing into metal ions.
a. State the name of this kind of reaction. (1)
b. Write ion-electron equations to show what happens to
the metal atoms during the corrosion of:
i. iron
ii. zinc (2)
SG Chem Topics 8 to 15 Page 18 Homework
Topic 12 – Homework 2
General Level
1. What is the name given to each of the following
processes?
a. Iron is dipped into molten zinc to give it a protective layer
against corrosion.
b. Scrap magnesium is used to protect an iron structure
against corrosion.
c. Electrolysis is used to coat iron with another metal. (3)
Credit Level
2. a. Write ion-electron equations for each of the reactions
which occur when iron is corroded by acid. (2)
b. Explain why galvanising does not protect iron
permanently from corrosion by acid. (1)
3. Three experiments were set up outside to investigate the
corrosion of “tin” cans. The three cans, A, B and C are
described below.
A: Iron can.
B. Iron can that is coated with tin.
C: Iron can that is coated with tin, but the tin coating is
scratched so exposing the iron underneath.
a. In which experiment will the iron not rust? Explain. (2)
b. In which experiment will the iron rust fastest?
Explain. (2)
4. Both zinc and tin are used to protect iron and steel
containers from corrosion. Metal dustbins are made from
iron which has been dipped into molten zinc; cans for
food are tin-plated.
a. Explain why zinc is preferred to tin for protecting
dustbins. (give two reasons). (2)
b. Explain why food cans are tin plated. (1)
SG Chem Topics 8 to 15 Page 19 Homework
Topic 13 – Homework 1
General Level
1. Consider the list of substances below:
polystyrene, rubber, nylon, polythene, bakelite,
starch, perspex, polypropene, terylene, wool
Put these in a table with the headings natural and
synthetic. (5)
2. Explain the purpose of each of the following:
a. The Teflon skin on some frying pans.
b. The PVC skin on some wallpapers.
c. The PVC covering on electric wires. (3)
3. Thermosetting plastics have different properties form
thermoplastics. Explain what is meant by:
a. Thermosetting plastic.
b. Thermoplastic (2)
Credit Level
4. Many plastics burn or smoulder to give off toxic fumes.
Name a plastic which can give off:
a. Carbon monoxide
b. Hydrogen chloride
c. Hydrogen cyanide (3)
SG Chem Topics 8 to 15 Page 20 Homework
Topic 13 – Homework 2
General Level
1. Consider the monomers below:
H H H H H H
C═C H C C C C H
H H H H H H
H H H H
C═C C H Cl C C Cl
H H H H H
ethane styrene
octane vinyl chloride
C3H8 C2F4
C2H4Br2 C3H5Cl
Draw a table and place each of the substances in the
appropriate column: able to undergo polymerisation or
not able to undergo polymerisation.
Credit Level
2. Polypropene is used to make kitchen items.
a. Name the monomer unit.
b. Draw the full structural formula of the monomer.
c. Draw the structure of part of the polypropene chain to
show how three monomer units have joined together.
(3)
SG Chem Topics 8 to 15 Page 21 Homework
Topic 13 – Homework 2 continued
Credit Level
3. The diagram shows part of the structure of a molecule of
Orion.
CH2 CH CH2 CH CH2 CH
CN CN CN
a. Draw the structural formula for the repeating unit in
Orion. (1)
b. Draw the structure of the monomer used to make
Orion. (1)
SG Chem Topics 8 to 15 Page 22 Homework
Topic 14 – Homework 1
General Level
1. Fertilisers are compounds which restore to the soil the
essential elements for plant growth.
a. Name the three elements which are restored to the
soil through use of fertilisers. (1)
b. Explain why woodland growth can be rapid while
farmland requires large quantities of fertilisers. (1)
2. The flow chart shows part of the nitrogen cycle.
Synthetic Nitrates
fertilisers in soil
Industrial process
Atmospheric Plants
nitrogen
Y Natural
X
fertilisers
Peas, beans, Animals
clover
a. Explain what is meant by:
i. Synthetic fertiliser.
ii. Natural fertiliser. (2)
b. Give an example of each. (1)
c. What is process X called? (1)
d. What types of living thing act on dead material to
bring about process Y? (1)
e. Crop yields have increased considerably in the last
50 years. Give a reason for this increase. (1)
f. Give an example of the effect of synthetic fertilisers
on river water. (1)
SG Chem Topics 8 to 15 Page 23 Homework
Topic 14 – Homework 1 continued
General Level
3. At the turn of the century a team of scientists led by Fritz
Haber discovered a cheap way to make an important
compound for the fertiliser industry. This is now called the
Haber process.
a. i. Name the compound which Haber produced. (1)
ii. Name the reactants in the process. (1)
iii. State where each reactant comes from. (1)
b. Which catalyst is used for the reaction? (1)
c. State two other conditions that are necessary for a
successful yield of the compound. (2)
Credit Level
4. Urea, CO(NH2) 2, and ammonium nitrate, NH4NO3, are
both fertilisers that supply nitrogen.
Find the most useful fertiliser by calculating the
percentage mass of nitrogen in each. (3)
SG Chem Topics 8 to 15 Page 24 Homework
Topic 14 – Homework 2
General Level
1. The manufacture of nitric acid is an important process in
the chemical industry.
Gas Z Platinum Oxides of nitrogen Nitric acid
air
a. What name is given to the process? (1)
b. Name gas Z. (1)
c. State the kind of chemical reaction taking place in the
first stage of the process (1)
d. What role does the platinum play? (1)
2. Nitrate fertilisers are made from nitric acid
Nitric acid + A ───> potassium nitrate
a. Name reagent A (1)
b. Name the other product of this reaction. (1)
c. Write a balanced equation for the reaction. (2)
d. Name the kind of reaction which is taking place. (1)
e. Give two reasons why nitrates are useful fertilisers.(1)
Credit Level
3. Ammonium sulphate is a fertiliser. Write a balanced
equation for the reaction of ammonia with sulphuric acid
to form ammonium sulphate. (2)
SG Chem Topics 8 to 15 Page 25 Homework
Topic 14 – Homework 2 continued
Credit Level
4. A student carried out two experiments on compound X.
Damp pH paper
Dilute
Sodium hydroxide
sulphuric acid
solution
Lime water
X X
Heat
A colourless gas was given off and A gas was given off that
the lime water became milky turned the pH paper blue
a. Name the gas given off in the first experiment. (1)
b. Name the gas given off in the second experiment (1)
c. Name compound X. (1)
d. Write a balanced equation to show the reaction of X
with sulphuric acid. (1)
SG Chem Topics 8 to 15 Page 26 Homework
Topic 14 – Homework 3
Credit Level
Calculations from Equations
1. CaCO3 ───> CaO + CO2
What mass of carbon dioxide is produced by the
decomposition of 10g of calcium carbonate? (3)
2. C2H4 + 3O2 ───> 2CO2 + 2H2O
What mass of water vapour is produced on burning 7g of
ethene? (3)
3. What mass of hydrogen is required to completely reduce
10g of copper (II) oxide to copper? (3)
4. What mass of hydrogen is obtained when 6.125g of
magnesium reacts with excess dilute hydrochloric
acid? (3)
5. What mass of propane is obtained when 7g of propene
(C3H6) reacts with hydrogen? (3)
SG Chem Topics 8 to 15 Page 27 Homework
Topic 15 – Homework 1
General Level
1. Starch and glucose are both carbohydrates.
a. Name the elements which are found in a
carbohydrate. (1)
b. Explain what is seen when a beam of light is passed
through
i. glucose solution
ii. starch in water (2)
Credit Level
2. Consider the list of carbohydrates below.
glucose, maltose, fructose, sucrose
a. Name the carbohydrates which are:
i. monosaccharides
ii. disaccharides (2)
b. Write the molecular formula for:
i. monosaccharides
ii. disaccharides (2)
c. Name the isomer of:
i. glucose
ii. maltose (2)
d. Which carbohydrate does NOT give a positive result
to the Benedicts test? (1)
3. A glucose monomer can be presented as shown:
HO ──── G ──── OH
a. Use the representation to draw three units in the
starch polymer chain. (1)
b. What kind of polymerisation takes place when starch
is formed from glucose? (1)
SG Chem Topics 8 to 15 Page 28 Homework
Topic 15 – Homework 2
General Level
1. The diagram below represents the process by which
energy is produced in animals.
a. Name the process. (1)
b. Name the gases X and Y. (1)
c. Give three examples of how the energy produced can
be used by animals. (3)
2. a. A carbohydrate was tested as shown in the diagram
below.
Test 1 Test 2
Warm water Iodine
solution
Carbohydrate +
benedicts solution Carbohydrate
Result: no change in the Result: iodine solution
colour of the Benedicts did not change colour.
solution.
Suggest a name for the carbohydrate which was
tested. (1)
SG Chem Topics 8 to 15 Page 29 Homework
Topic 15 – Homework 2 continued
General Level
2. b. Test 3 Test 4
hot water iodine
solution
carbohydrate
in water + carbohydrate
dilute
hydrochloric
acid
Result: after the solution Result: iodine solution
was neutralised, Benedicts turned blue/black.
solution gave an orange
precipitate.
i. Name the carbohydrate used in tests 3 and 4. (1)
ii. Name the carbohydrate produced by the
reaction in test 3. (1)
3. Study the flow diagram below and answer the questions
which follow:
glucose
solution
fermenter fermented separator
liquid
yeast
gas X waste alcohol
liquid
a. Name gas X. (1)
b. What kind of substance, present in yeast, acts as a
catalyst for the reaction? (1)
c. Name the alcohol produced by this process.
d. How is the alcohol separated from the waste liquid?
(1)
SG Chem Topics 8 to 15 Page 30 Homework
Topic 15 – Homework 2 continued
Credit Level
4. The production of ethanol from glucose is normally
carried out at a temperature around 40°C.
a. Write a balanced chemical equation for the
reaction. (2)
b. i. Would the reaction be speeded up by boiling? (1)
ii. Explain your answer to b. i.. (1)
c. Explain why there is a limit to the concentration of
ethanol obtained in this reaction. (1)
SG Chem Topics 8 to 15 Page 31 Homework