Chemistry Assignment For G 12b, 12c & 12d
Chemistry Assignment For G 12b, 12c & 12d
Chemistry Assignment For G 12b, 12c & 12d
SECTION A
1|Page
5. How many moles of oxygen molecules are there in 64 grams of oxygen,
O2?
A. 2 moles B. 4 moles C. 8 moles D.16
6. Dilute hydrochloric add reacts with both magnesium oxide and calcium
carbonate.
What is common about these reactions?
A. Carbon dioxide is produced
B. Water is produced
C. Water vapour is condensed
D. A white precipitate is formed
8. The graph below shows the rate of reaction between a metal and a dilute
acid.
10. Which of the following alkanes has the highest boiling point?
2|Page
A. CH4 B. C2H6 C. C3H8 D. C4H10
SECTION: B
B1. (a) Define a hydrocarbon.
………………………………………………………………………………………
…………………………………………………………………………………… [1]
(b) State the difference between saturated hydrocarbons and unsaturated
hydrocarbon.
………………………………………………………………………………………
………………………………………………………………………………………
………………………………………………………………………………………
…………………………………………………………………………………. [2]
(c) Organic compounds form homologous series.
Give two characteristics of members of any homologous series.
……………………………………................................................................
……………………………………………………………………………… [2]
(d) (i) Draw the structure of an alkane with two carbon atoms in the molecule.
[2]
(ii) Calculate the percentage by mass of hydrogen in this alkane.
……………………………………………………………...........................
…………………………………………………………………………… [2]
[Total: 9 marks]
3|Page
B2. The diagrams below show the electron arrangement in the outer shell of five
elements A to E.
All elements are from Period 3 of the Periodic Table.
(a) Put the letters A to E in the table to shows which elements are metals and
which are non-metals.
Metals Non-metals
[5]
…………………………………………………………………………… [1]
4|Page
SECTION: C
Answer all questions from this section
C1. The table below shows the results of the production of hydrogen in the reaction
between zinc granules and dilute hydrochloric acid at 25oC.
Volume (cm3) 0 5.0 10.0 13.0 15.5 18.5 19.5 19.5 19.5
Time (Min) 0 0.6 1.5 2.3 3.0 4.4 5.7 7.0 7.5
(a) Plot a graph of volume against time for the reaction [3]
(b) Calculate the average rate of the reaction during the first 3
minutes [2]
(c) Use the graph to determine the volume of gas collected after 5 minutes
[2]
(d) On the same graph, sketch a curve you would expect if powdered
zinc were used instead of zinc granules. Label this curve P [1]
(e)How long did it take for the reaction to end? [1]
(f) Mention factors you would employ to increase the rate of production of
the gas. [3]
(g), Explain briefly how each of the mentioned factors above increases the
rate of production of the gas.
[6]
[Total: 18 marks]
C2. (a) Work out the relative formula mass, Mr of the following:
(i) Ca(HCO3)2 (ii) Al2(SO4)3 [2]
(b) When water containing dissolved calcium hydrogen carbonate is boiled, the
calcium hydrogen carbonate decomposes according to the equation below:
Ca(HCO3)2(aq) CaCO3(s) + H2O (l) + CO2(g)
[Total: 5 marks]
5|Page
C3. A piece of Magnesium ribbon was made to react with dilute hydrochloric acid. The
volume of the hydrogen gas collected in a syringe was measured at intervals. The results
are shown below.
Gas syringe
RESULTS
Time/minutes 0 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 4.5 5.0 5.5 6.0
Volume of hydrogen gas 0 8 14 20 25 35 33 36 38 39 40 40 40
3
(cm )
(a) Write a balanced chemical equation for the reaction between magnesium and
dilute hydrochloric acid (include state symbols). [3]
(b) Plot a graph of the results (volume against time) on the graph paper provided. [3]
(c) Which result should be rejected as being an error? [1]
(d) What was the maximum volume of hydrogen produced in this reaction? [1]
(e) From the graph, how can you tell when the reaction came to an end? [1]
(d) What is the average rate of this reaction? [1]
[Total: 10 marks]
6|Page
NOTES
Organic chemistry
Definition: Organic chemistry is the study of carbon compounds except carbonates,
carbon monoxide, carbon dioxide, carbon disulphide etc.
Common terms used
1. Organic compounds
Organic compounds are compounds which contain carbon except carbonates, carbon
monoxide, carbon dioxide, carbon disulphide etc.
2. Hydrocarbon
A hydrocarbon is a compound which consists of the elements carbon and hydrogen only,
Example
Hydrocarbon Formula
Methane
Ethene
Ethyne
3. Homologous series
A homologous series is a family of similar organic compounds
Each member in a family is called homologue
Characteristics of the homologous series
(a) Members in the family show a gradual change in physical properties i.e.
change from gas to liquid and solid as the carbon chain increases.
(b) Members in the family have similar methods of preparation
(c) Members in the family have similar chemical properties because they have
the same functional group.
(d) Members in the family can be represented by the general molecular formula:
Example
Organic family General molecular formula
Alkanes
Alkenes
Alkynes
Alcohols (Alkanols)
Esters
7|Page
4. Functional group
A functional group is a group is a group which determines the chemical properties of
organic compounds
Organic family Functional group Name of functional group
Alkanes ─C─C─ Single carbon – carbon covalent bond
Alkenes C=C Double carbon – carbon covalent bond
Alkynes C≡C Triple carbon – carbon covalent bond
Alkanols ( alcohols) ─ OH Hydroxyl group
─ COOH
or
Alkanoics (carboxylic Carboxyl group
acids)
8|Page
Suffix Organic family
ane Alkanes
ene Alkenes
yne Alkynes
anol Alcohols
anoic Carboxylic acids
anoate Esters
Alkanes
Alternative term: Saturated hydrocarbons
General molecular formula: where n = 1, 2, 3, 4…….
Alkanes have single carbon – carbon covalent bonds between carbon atoms.
They are called saturated hydrocarbons because they have the required (maximum)
number of hydrogen atoms. They end with ane
Examples of alkanes
9|Page
Preparation of methane
Methane can be prepared by heating a mixture of anhydrous sodium ethanoate,
COONa, and soda lime (sodium hydroxide), NaOH.
Reaction: COONa(s) + NaOH(s) → CH4(g) + Na2CO3(s)
Diagram:
(c) In a very limited supply of air (incomplete combustion), alkanes react with oxygen to
form carbon and water
Example
C3H8 + 2O2 → 3C + 4H2O
10 | P a g e
2. Substitution reaction
A substitution reaction is a reaction in which one atom or group of atoms in a molecule
is replaced by another.
Alkanes undergo substitution reactions with halogens in the presence of ultraviolet light.
Example
Halogenation of methane
Methane can react with chlorine gas in the presence of sunlight to form chloromethane
and hydrogen chloride.
CH4(g) + Cl2(g) → CH3Cl(g) + HCl(g)
Conditions
1. Temperature: 200oC
2. Catalyst: Sunlight (ultraviolet light)
Isomerism of alkanes
Isomerism is the existence of compounds with the same same molecular formula
but different structural formula Isomers
Isomers are compounds which have the same molecula formula but different structural
formula.
The International Union for Pure and Applied Chemistry (IUPAC) rules for naming
alkanes
11 | P a g e
• Number the carbon atoms in the longest chain chosen starting from the end that
gives the smaller set of numbers nearer the branched methyl group
• Write the number of carbon atom at which the branched methyl group is
attached to the main chain in alphabetical order.
• Put a comma after each group number and a hyphen between the group number
and the methyl group.
• Name the compound as a derivative of the normal alkane having the same
number of carbon atoms as in the longest chain chosen.
Molecular formula:
IUPAC name: Normal butane
Molecular formula:
IUPAC name: 2 – methyl propane
12 | P a g e
Molecular formula:
IUPAC name: Normal pentane
Molecular formula:
IUPAC name: 2 – methyl butane
Molecular formula:
IUPAC name: 2, 2 – dimethyl propane
Exercise
1. Draw the structure of the compound with the IUPAC name; 2, 3, 4, 4 – tetra
methylpentane
Cracking of alkanes
Cracking is the breaking down of large hydrocarbon molecules into simpler and smaller
molecules.
Alkanes break down to produce alkenes, short chain alkanes and in some cases hydrogen
gas.
Types of cracking
13 | P a g e
1. Thermal cracking
This is where heat is used to break down large molecules into smaller ones.
Example
C2H6 → C2H4 + H2
2. Catalytic cracking
This is where both heat and a catalyst are usedto break down large molecules into
smaller ones.
Common catalysts used include aluminium oxide (Al2O3) and silica (SiO2).
Example
Conditions
Importance of cracking
1. It is used in the production of raw materials for petrol chemicals like ethene and
hydrogen.
Hydrogen is used in making plasitics and margarine.
2. It is used in the production of petrol.
Exercise
Fuels
14 | P a g e
A fuel is a substance which burns in air to produce useful energy.
Sources of fuels
15 | P a g e
Fraction Number of carbon atoms Use
Petroleum gases C1 – C4 Used in camping stoves and cookers as
bottled gas
Petrol (gasoline) C4 – C10 Used as a fuel in internal combustion
engines in vehicles
Kerosine ( paraffin) C10 – C17 Used as a fuel in jets
Used in paraffin lamps for lighting
Used in paraffin lamps for cooking
Diesel oil (gas oil) C17 – C20 Used as a fuel in diesel engines like trains,
hammer mills, tractors, lorries
Lubricating oil C20 – C30 Used as a lubricant in machines to reduce
friction
Fuel oil C30 – C40 Used as a fuel in ships, power stations and
industrial machinary
Paraffin waxes C40 – C50 Used in making waxes, polishes and wax
papers
Bitumen (residue) C50 upwards Used to tar roads
Used as a roofing material
Note
1. Petroleum gases have the smallest boiling point and have the smallest relative
molecular mass.
2. Bitumen has the highest boiling point and have the largest relative molecular
mass. In addition, bitumen has the longest chain.
3. Octane is the main component of petrol
Exercise
16 | P a g e
1. Crude oil, a mixture of hydrocarbons, can be separated by fractional distillation. The
diagram below shows a fractionating tower and different fractions obtained from crude
oil
Methane reacts with steam to form carbon monoxide and hydrogen gas.
Conditions
1. Temperature: 200oC
2. Catalyst: Nickel metal
Exercise
17 | P a g e
1. Hydrogen can be manufactured from methane using a nickel catalyst as shown in the
diagram below
Alkenes
C= C
They are called unsaturated hydrocarbons because they have a double bond between
carbon atoms.
They have two hydrogen atoms less than their corresponding alkanes
18 | P a g e
Examples of alkenes
Alkene Molecular formula Structural formula Condensed formula Mr
19 | P a g e
There are two methods used to prepare ethene.
This is where a catalyst is used to break down large hydrocarbon molecules into smaller
ones.
Conditions
1. Temperature: 600oC
2. Catalyst: Aluminium oxide, Al2O3
Note: The broken pot can act as a catalyst.
2. Dehydration of ethanol
Ethene can be prepared by the dehydration of ethanol using concentrated sulphuric acid
as a dehydrating agent.
Conditions
20 | P a g e
1. Temperature: 180oC
2. Dehydrating agent: Concentrated sulphuric acid.
There are two ways you could test a hydrocarbon, to see whether it is an alkane or
Result: The brown colour of bromine disappears immediately. In other words, alkenes
decolorize bromine water.
Explanation: When ethene reacts with bromine water, the colourless compound (liquid)
called 1, 2 – dibromoethane is formed.
Note
When an alkane is shaken with bromine water, there is no reaction. Alkanes do not
undergo addition reactions because they are saturated.
Test 2: Add acidified potassium per manganate (VII) solution to the hydrocarbon.
Result: The purple colour of potassium per manganate (VII) turns colourless if an alkene
is present.
Alkenes are more reactive than alkanes because the double bond opens up to allow
chemical reactions.
1. Combustion
21 | P a g e
Alkenes react with oxygen to form carbon dioxide and water.
Example
2. Addition reactions
Alkenes react with hydrogen to form corresponding alkanes. Hydrogen makes the
unsaturated compounds to become saturated. Ethene reacts with hydrogen to form ethane
Conditions
1. Temperature: C
2. Catalyst: Nickel metal
22 | P a g e
Ethene reacts with steam to in the presence of phosphoric acid to form ethanol.
Conditions
1. Temperature: C
2. Catalyst: Phosphoric acid,
3. Pressure: 65 atmospheres
Uses of ethene
Exercise
23 | P a g e