WAEC SSCE - Chemistry - 2001
Question 1 Report
Which of the following reactions represents the change that occurs when a photographic film is exposed to sunlight?
Answer Details
When a photographic film is exposed to sunlight, the silver halide grains in the film emulsion are converted to metallic silver. This process involves the reduction of silver ions (Ag+) to neutral silver atoms (Ag) by the electrons (e-) produced by the exposure to light. Therefore, the correct reaction that represents the change that occurs when a photographic film is exposed to sunlight is: Ag+ + e- → Ag
Question 2 Report
If 10 cm 3 of distilled water is added to 10 cm3 of an aqueous salt solution, the concentration of the solution
Answer Details
If 10 cm3 of distilled water is added to 10 cm3 of an aqueous salt solution, the total volume of the resulting solution is 20 cm3. However, the amount of solute (the salt) in the solution remains constant, while the amount of solvent (the water) increases. Therefore, the concentration of the solution decreases since the same amount of solute is now present in a larger volume of solution. So, the correct option is: the concentration decreases.
Question 3 Report
Which of the following polymers contains nitrogen?
Answer Details
Nylon is the polymer that contains nitrogen. Nylon is a synthetic polymer that contains amide linkages in its structure. These amide linkages are formed between the amine group (-NH2) of one monomer and the carboxylic acid group (-COOH) of another monomer, resulting in the formation of a long chain polymer with repeating units of -(NH-[CH2]n-CO)-. The presence of the amide group in nylon gives it unique properties such as high strength and elasticity.
Question 4 Report
What will happen if more heat is applied to the following system at equilibrium? X2(g) + 3Y 2(g) ⇌ 2XY3(g); ∆H =-kJmol -1
Answer Details
Question 5 Report
It can be concluded that gastric juice
Answer Details
Gastric juice is a digestive fluid secreted by the stomach. It is primarily composed of hydrochloric acid, which makes it very acidic with a pH value of about 2. Additionally, gastric juice contains enzymes such as pepsin, which is responsible for breaking down proteins. Therefore, it can be concluded that gastric juice contains enzymes and is acidic. It is not a mixture of substances, and it does not have a pH value of 7, which is neutral.
Question 6 Report
In the electrolysis of CuSO4(aq) using copper electrodes, the reaction at the anode is
Answer Details
During the electrolysis of copper sulfate (CuSO4), the copper anode loses mass as copper atoms are oxidized to form copper ions that enter the solution. This means that the reaction at the anode is the dissolution of the copper electrode. Therefore, the correct option is "dissolution of copper electrode."
Question 7 Report
Which of the following substances increases in mass when heated in air?
Answer Details
Question 8 Report
Which of the following features of a human skeleton can be determined by carbon-dating?
Answer Details
Carbon dating is a method used to determine the age of organic materials, such as bones and teeth. This method is based on the fact that carbon-14, a radioactive isotope of carbon, decays at a known rate over time. As living organisms take in carbon-14 during their lifetime, the amount of carbon-14 in their bones and teeth can be used to determine the approximate age of the sample. Therefore, of the options given, only the age of a human skeleton can be determined by carbon-dating. The other features such as height, mass, and race cannot be determined by carbon-dating.
Question 9 Report
Acidic industrial waste can be treated with
Answer Details
Acidic industrial waste can be treated with lime. Lime is an alkaline substance that can be used to neutralize acidic waste by a process called neutralization. In this process, the lime reacts with the acid to form a salt and water, resulting in a neutral pH. This neutralization reaction is an important step in the treatment of industrial waste, as acidic waste can be harmful to the environment and living organisms. Brine, water, and ethanol are not commonly used for treating acidic waste.
Question 10 Report
CuSO4 5H2O can be obtained from an aqueous solution of copper (ll) tetraoxosulphate (VI) by
Answer Details
CuSO4 5H2O can be obtained from an aqueous solution of copper (ll) tetraoxosulphate (VI) by crystallization. Crystallization is a process of separating a solid product from a liquid by allowing the liquid to evaporate under controlled conditions. In this case, an aqueous solution of copper (II) tetraoxosulphate (VI) can be heated to form a saturated solution. The solution is then cooled slowly to allow the formation of CuSO4 5H2O crystals. These crystals can be collected by filtration to obtain the desired product. Therefore, the correct option is "crystallization".
Question 11 Report
Waste plastics accumulate in the soil and pollute the environment because plastic materials are
Answer Details
The accumulation of waste plastics in the soil and the environment is mainly due to the fact that plastic materials are non-biodegradable. This means that they cannot be broken down by natural biological processes, unlike organic materials such as paper or food waste. Plastics are made up of long chains of polymers that do not readily decompose, and thus persist in the environment for a long time, causing pollution. Plastics are also typically insoluble in water, making it difficult for them to dissolve and be removed by water-based processes. While some plastics are flammable, they are not easily affected by heat in the sense of breaking down or decomposing quickly, and may actually release harmful gases when burned.
Question 12 Report
The presence of unpaired electrons in an atom of a transition metal gives rise to
Answer Details
The presence of unpaired electrons in an atom of a transition metal gives rise to paramagnetism. Paramagnetism is a type of magnetism that occurs when certain materials are placed in an external magnetic field. When a transition metal atom has unpaired electrons in its outermost energy level, it can become magnetized and attracted to an external magnetic field. This is because the unpaired electrons can align their spins with the external magnetic field, causing the atom to become magnetized. Therefore, the presence of unpaired electrons in an atom of a transition metal is responsible for its paramagnetic behavior.
Question 14 Report
Elements which belong to the same group in the Periodic Table are characterized by
Answer Details
Elements which belong to the same group in the Periodic Table are characterized by the presence of the same number of outermost electrons in the respective atoms. The groups are the columns in the periodic table, and elements within the same group have similar chemical and physical properties. This is because they have the same number of valence electrons, which are the electrons involved in chemical bonding. As a result, they tend to react similarly with other elements and form similar types of compounds. Therefore, the correct option is (b): presence of the same number of outermost electrons in the respective atoms.
Question 15 Report
In which of the reactions represented by the following equations is HNO3 behaving as a typical acid?
Answer Details
Question 16 Report
Sugars can be hydrolyzed at room temperature by the action of
Answer Details
Sugars are carbohydrates that can be broken down by hydrolysis, which involves breaking down the glycosidic bond between the sugar units. Hydrolysis of sugars can occur by the action of different agents. Mineral acids and strong bases can both catalyze the hydrolysis of sugars, but they require high temperatures to work efficiently. Enzymes, on the other hand, are biological catalysts that can catalyze the hydrolysis of sugars at room temperature, with high specificity and efficiency. Enzymatic hydrolysis of sugars involves the action of specific enzymes that recognize and break down specific types of glycosidic bonds. Oxidants, which are substances that can accept electrons in a chemical reaction, are not typically used to hydrolyze sugars.
Question 17 Report
What is oxidized in the reaction represented by the following equation? 3CU + 8HNO3 → 3Cu(NO3)2 + 2NO + 4H2O
Answer Details
In the given reaction, copper is oxidized because its oxidation state increases from 0 in Cu to +2 in Cu(NO3)2. Oxidation is defined as the loss of electrons or an increase in oxidation state. Here, copper loses electrons and its oxidation state increases, hence it is oxidized. Therefore, the correct answer is copper.
Question 18 Report
Which of the following statements about ideal gases is/are correct? 1. The cohesive forces between their particles are negligible ll. The have no definite volume but occupy the volume of their containers III. They are not compressible IV. Their particles collide with loss of energy
Question 19 Report
What is the function of H2SO4 in the following reaction? C12
H22O11 conc. H24 12C + 11H2O
Answer Details
The function of H2SO4 in the given reaction is that of a dehydrating agent. The concentrated sulfuric acid (H2SO4) is used in this reaction to remove the water (H2O) molecule from the reactant molecule C12H22O11 (sucrose). The removal of a water molecule from a molecule is known as dehydration. Therefore, in this reaction, H2SO4 acts as a dehydrating agent, which removes water from the reactant molecule and helps to form carbon (C) and water (H2O) as products.
Question 20 Report
Which of the following would dissolve in warm dilute H2SO4 without effervescence, to give a blue solution?
Answer Details
Question 21 Report
Which of the following compounds is covalent?
Answer Details
Among the given compounds, CH4 is covalent. Covalent compounds are formed when two or more non-metal atoms share electrons to form a molecule. CH4 is methane, which is a simple organic compound made up of one carbon and four hydrogen atoms. Both carbon and hydrogen are non-metals, and they share electrons to form four covalent bonds, resulting in a stable molecule. The other three compounds, CaCI2, MgO, and NaN, are all ionic compounds, which are formed by the transfer of electrons between a metal and a non-metal.
Question 22 Report
Which of the following decreases when a given mass of gas is compressed to half its initial volume?
Answer Details
Question 23 Report
A feasible cell was constructed by joining the two half cells below. Cu2+ (aq) + 2e- → Cu(s) Eo = - 0.76 V. What is the standard e.m.f. of the cell?
Question 24 Report
The conclusion from Rutherford's from radioactive substance alpha-scattering experiment is that
Answer Details
The conclusion from Rutherford's alpha-scattering experiment is that atoms are mostly empty space with a small, dense, positively charged nucleus at the center. This was determined by observing that alpha particles, which are positively charged, were mostly able to pass through the gold foil with little to no deflection, but occasionally were deflected at large angles. This led to the conclusion that most of the atom's mass and positive charge is concentrated in a small, dense nucleus at the center, with the electrons orbiting around it.
Question 25 Report
The atom of an element X combines with aluminium (13AI)?
Answer Details
The correct answer is AI 2X 3. This is because when the atom of an element X combines with aluminium (13AI), it forms an ionic compound. The formula for ionic compounds is determined by balancing the charges of the ions involved. Aluminium has a charge of 3+ while the atom of element X has a charge of 2-. To balance the charges, two atoms of element X are required for every three aluminium atoms. The resulting formula for the compound is AI 2X 3.
Question 26 Report
Given that the order of reactivity of four metals is P>Q>R>S, which of the following reactions is feasible?
Answer Details
Feasible reactions between two metals occur when the metal higher in the reactivity series displaces the metal lower in the reactivity series from its compound. Based on the given order of reactivity (P>Q>R>S), feasible reactions will occur between P and Q, R and S, and P and S. Therefore, the only feasible reaction from the options provided is: Q + S+ → S + Q+
Question 27 Report
Equal amounts of marble chips are reacted separately with 100cm3 of hydrochloric acid of different concentrations . if all the marble chips reacted, which of the following remained the same in each case?
Question 28 Report
Which of the following substances decomposes when an electric current is passed through it?
Answer Details
Out of the given options, tetrachloromethane is the substance that decomposes when an electric current is passed through it. Tetrachloromethane, also known as carbon tetrachloride, is a covalent compound with the chemical formula CCl4. It is a non-conductor of electricity in its pure form, but when it is mixed with small amounts of impurities, it becomes a conductor of electricity. When an electric current is passed through it, tetrachloromethane undergoes electrolysis, which breaks down the C-Cl bonds and forms various products, including chlorine gas and phosgene gas. On the other hand, glucose solution, zinc rod, and hydrochloric acid do not decompose when an electric current is passed through them. Glucose is a covalent compound that does not dissociate into ions in solution, so it cannot undergo electrolysis. Zinc is a metal and a good conductor of electricity, but it does not undergo any significant chemical reaction when an electric current is passed through it. Hydrochloric acid is an aqueous solution of hydrogen chloride, which dissociates into H+ and Cl- ions in solution. However, it is not a good conductor of electricity because the concentration of ions is relatively low.
Question 29 Report
Which of the following pairs of reagents reat to produce hydrogen?
Answer Details
The pair of reagents that react to produce hydrogen is: Magnesium and dilute tetraoxosulphate (VI) acid. When magnesium is added to dilute tetraoxosulphate (VI) acid, hydrogen gas is produced as one of the products. This is a classic example of a single-displacement reaction, where the more reactive metal (magnesium) displaces the less reactive hydrogen from the acid. The other options do not produce hydrogen gas upon reaction.
Question 30 Report
A gas was evolved when a sample of gastric juice reacted with sodium trioxocarbonate (IV) . The gas evolved was
Answer Details
The gas evolved when a sample of gastric juice reacts with sodium trioxocarbonate (IV) can be determined by identifying the reaction taking place. Gastric juice contains hydrochloric acid (HCl), and when it reacts with sodium trioxocarbonate (IV) (Na2CO3), carbon dioxide (CO2) gas is evolved. This is because the reaction between hydrochloric acid and sodium trioxocarbonate (IV) produces carbon dioxide, sodium chloride, and water as products. The balanced equation for this reaction is: 2HCl + Na2CO3 → CO2 + NaCl + H2O Therefore, the correct answer is CO2.
Question 31 Report
A reaction is represented by the equation below. A2(g) + B2(g) 2AB(g); ∆H = +X kJmol-1 Which of the following statements about the system is correct?
Answer Details
Question 32 Report
If a metal R forms a compound with the formula R(NO3)2 the formula of its tetraoxosulphate (VI) is
Answer Details
Question 34 Report
A major factor coonsidered in selecting a suitable method for preparing a simple salt is its
Answer Details
When preparing a simple salt, one of the major factors to consider is its solubility in water. This is because the method used for preparation should be able to dissolve the necessary reactants in water to form a solution that can be further processed to yield the desired salt. The solubility of a salt in water determines the concentration of the reactants in the solution and affects the rate and completeness of the chemical reaction. Hence, solubility plays a critical role in selecting a suitable method for preparing a simple salt.
Question 35 Report
A substance is said to be hygroscopic if it absorbs?
Answer Details
A substance is said to be hygroscopic if it absorbs moisture from the atmosphere without dissolving. Hygroscopic substances have the ability to attract and retain water molecules from the air around them, which can lead to their physical properties being altered. This can include changes in texture, shape, and size. Some examples of hygroscopic substances include salt, sugar, and certain types of paper.
Question 36 Report
What does ∆H represent in the following equation ? Cl(g) + e- → CI- (g); ∆H = - 363 kJ mol-1
Answer Details
In the given equation, ∆H represents the Electron affinity. Electron affinity is the energy change that occurs when an atom in the gas phase gains an electron to form a negative ion. The negative value of ∆H in the equation indicates that energy is released when an electron is added to the chlorine atom to form a chloride ion.
Question 37 Report
A visible change is observed when a strip of iron is placed in an aqueous solution of
Answer Details
When a strip of iron is placed in an aqueous solution of CuSO4, a visible change is observed. This is because copper ions in the CuSO4 solution gain electrons from the iron strip and are reduced to metallic copper, which is deposited on the iron strip. At the same time, iron atoms on the strip lose electrons and are oxidized to iron(II) ions, which dissolve in the solution. The overall reaction is: Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s) The visible change observed is the deposition of metallic copper on the iron strip, which appears as a reddish-brown coating. This process is known as a displacement reaction, where a more reactive metal (in this case, iron) displaces a less reactive metal (copper) from its salt solution.
Question 38 Report
A concentrated solution containing H+, Cu2+,OH- and CI- was electrolysed using platiunm electrodes which of the ions will be discharged at the cathods?
Answer Details
Question 39 Report
What volume of hydrogen will be produced if 100cm3 of ammonia is completely decomposed at constant temperature and pressure? The equation for the reaction is 2NH3(g) → N2(g) + 3H2(g)
Answer Details
From the balanced chemical equation, we know that 2 moles of NH3 will produce 3 moles of H2. Therefore, to calculate the volume of H2 produced, we need to first find the number of moles of NH3 in 100cm3: 1 mole of any gas at room temperature and pressure (RTP) occupies a volume of 24dm3 (24000cm3). Therefore, the number of moles of NH3 in 100cm3 can be calculated as follows: 100cm3 = 100/1000 = 0.1dm3 0.1dm3 of NH3 at RTP = 1/24 moles (since 24dm3 = 1 mole) Therefore, the number of moles of NH3 in 100cm3 = (1/24) x 0.1 = 0.00417 moles (to 3 significant figures) Since 2 moles of NH3 produce 3 moles of H2, we can calculate the number of moles of H2 produced as follows: Number of moles of H2 = (3/2) x 0.00417 = 0.00625 moles (to 3 significant figures) Finally, we can use the ideal gas law to calculate the volume of H2 produced: PV = nRT where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. Since the temperature and pressure are constant, we can write: VH2 / nH2 = VNH3 / nNH3 where VH2 and nH2 are the volume and number of moles of H2, and VNH3 and nNH3 are the volume and number of moles of NH3. Substituting the values we have calculated: VH2 / 0.00625 = 0.1 / (1/24) VH2 = 0.00625 x (1/0.0417) x 24 = 150cm3 Therefore, the volume of hydrogen produced is 150cm3.
Question 40 Report
P Total = F1 + P2 + P 3 + .........Pn' where P Total is the pressure of a mixture of gasses. The equation above is an expression of
Answer Details
The equation PTotal = F1 + P2 + P 3 + .........Pn' is an expression of Dalton's law. Dalton's law states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases in the mixture. In other words, the total pressure exerted by a mixture of gases is equal to the sum of the pressures that each gas would exert if it were present alone in the same container at the same temperature.
Question 41 Report
The gas given off when NH4Cl is heated with an alkali is
Answer Details
When NH4Cl is heated with an alkali, it undergoes a chemical reaction known as the Hofmann's degradation reaction, which produces ammonia gas (NH3). The reaction is represented as: NH4Cl + NaOH → NaCl + H2O + NH3 Therefore, the correct answer is NH3.
Question 42 Report
Calculate the mass of sodium hydroxide in 5.00 dm3 of a 0.125 mol dm-3 solution [NaOH = 40 g mol]
Answer Details
To calculate the mass of sodium hydroxide in 5.00 dm3 of a 0.125 mol dm-3 solution, we need to use the formula: mass = molarity x volume x molecular weight where: - molarity = 0.125 mol dm-3 (given) - volume = 5.00 dm3 (given) - molecular weight of NaOH = 40 g mol-1 (given) Substituting the values into the formula, we get: mass = 0.125 mol dm-3 x 5.00 dm3 x 40 g mol-1 mass = 25.0 g Therefore, the mass of sodium hydroxide in 5.00 dm3 of a 0.125 mol dm-3 solution is 25.0 g. The correct option is (d).
Question 43 Report
Which of the following salt solutions will have a pH greater than 7?
Question 44 Report
One of the products of combustion of pentane in excess air is
Answer Details
One of the products of combustion of pentane in excess air is carbon (IV) oxide. During combustion, pentane reacts with oxygen from the air to produce carbon dioxide and water. The balanced chemical equation for the combustion of pentane is: C5H12 + 8O2 → 5CO2 + 6H2O This means that for every molecule of pentane that reacts, five molecules of carbon dioxide and six molecules of water are produced. Since carbon dioxide is a type of carbon (IV) oxide, it is one of the products of combustion of pentane in excess air.
Question 45 Report
Consider the following equation: Ag+ (aq) + CI-(aq) → Ag+CI- (s) ; ∆H = _65.7 kJmol-1. From the equation, it can be deduced that
Answer Details
The given equation is a chemical equation that represents a reaction between silver ion (Ag+) and chloride ion (CI-) to form silver chloride (Ag+CI-). The value of enthalpy change (∆H) is given as -65.7 kJmol-1, which indicates that the reaction is exothermic, i.e., heat is evolved during the reaction. Thus, the correct option is "a solid is formed and heat is evolved."
Question 46 Report
Hydrogenation of butene yields
Answer Details
The hydrogenation of butene involves the addition of hydrogen gas to the double bond of butene molecule. This reaction is a type of addition reaction, where two reactants combine to form a single product. The product of the hydrogenation of butene is butane. This is because the addition of hydrogen to the double bond of butene saturates the carbon atoms, and forms a single bond between them, resulting in a straight-chain alkane. Therefore, the correct answer is "butane".
Question 47 Report
A mixture of calcium chloride and calcium trioxocarbonate (IV) in water can be separated by
Answer Details
A mixture of calcium chloride and calcium trioxocarbonate (IV) in water can be separated by filtration. Filtration is a separation technique that separates solids from liquids using a porous material or a filter. Calcium trioxocarbonate (IV) is insoluble in water while calcium chloride is soluble in water. When the mixture is passed through a filter, calcium trioxocarbonate (IV) will be left behind as a residue while the filtrate will contain calcium chloride in water. Therefore, filtration can be used to separate the two components of the mixture.
Question 48 Report
What is responsible for metallic bonding?
Answer Details
Metallic bonding is responsible for the unique properties of metals, such as their malleability, ductility, and conductivity. It occurs due to the attraction between the positively charged atomic nuclei and the delocalized cloud of electrons surrounding them. In metallic bonding, the valence electrons are not held tightly by any one atom but are free to move throughout the metal lattice. This allows for the sharing of electrons between many atoms, creating a cohesive and stable structure. Therefore, the correct answer is "Attraction between the atomic nuclei and cloud of electrons."
Question 49 Report
A sheet of paper is placed in the path of a beam from a radioactive source. The emissions that pass through the paper consist of
Answer Details
Question 50 Report
What is the oxidation number of nitrogen in AI(NO3)3?
Answer Details
In AI(NO3)3, the compound has a total charge of 0 because aluminum has a charge of +3 and nitrate (NO3) has a charge of -1. Since there are three nitrate ions, their total charge is -3. Therefore, the oxidation number of nitrogen can be calculated as follows: AI(NO3)3 Aluminum = +3 Oxygen (O) in NO3 = -2 Nitrogen (N) in NO3 = x The sum of the oxidation numbers must equal the charge of the compound (0). +3 + 3(-2) + 3x = 0 -6 + 3x = 0 3x = 6 x = +2 Therefore, the oxidation number of nitrogen (N) in AI(NO3)3 is +5.
Question 51 Report
Which of the following constitutes an advantage in the use of hard water?
Answer Details
Hard water is water that contains dissolved minerals such as calcium and magnesium. These minerals can provide health benefits and contribute to the formation of strong bones, which is an advantage. However, the other options listed in the question are disadvantages of hard water. When hard water reacts with soap, it forms scum that reduces the effectiveness of cleaning. Furring of kettles is the buildup of mineral deposits that reduces efficiency and increases energy consumption. Blockage of water pipes can lead to reduced water flow and increased maintenance costs.
Question 52 Report
Benzene produces more soot than ethene on burning because benzene
Question 53 Report
(a) State three characteristic properties of
(i) electrovalent compounds;
(ii) alpha particles
(iii) catalysts
(b)(i) Write the electronic configuration of silicon (atomic number 14) and state the group to which it belongs in the Periodic Table.
(ii) State the type of chemical bonding between silicon and oxygen in SiO\(_2\)
(iii) A chip used in a microcomputer contains 5.72 x 10\(^{-3}\)g of silicon, calculate the number of silicon atoms in the chip.
[Si = 28; Avogadro constant = 6.02 x 10\(^{23}\) mol\(^{-1}\)]
(c) An element X belongs to the same group as sodium but is more reactive.
(i) Suggest with reason whether X would be a reducing or oxidizing agent.
(ii) What would be a suitable method of storing X in the laboratory?
(iii) Describe briefly what would be observed if a small piece of X were dropped into a trough of cold water which had been coloured with red litmus.
(iv) Write an equation to show how the oxide of X would react with dilute HCI.
(v) Suggest the likely colour of the salts of X
Question 54 Report
(a)(i) Explain what is meant by acid anhydride and give one example
(ii) State three chemical properties of hydrochloric acid.
(b) Explain each of the following observations:
(i) Tetraoxosulphate (VI) acid can form two types of salts unlike trioxonitrate (V) acid.
(ii) Copper and iron react with concentrated H\(_2\)SO\(_4\) but only one of them reacts with the dilute acid.
(iii) On adding dilute H\(_2\)SO\(_4\) separately to zinc dust and zinc granules of the same mass, the dust produced more vigorous effervescence.
(c)(i) Define activation energy.
(ii) Sketch and label an energy profile diagram for the following reaction: A + B --> C + D; AH = xkJmol\(^{-1}\)
(iii) Explain why the heat of reaction of the mineral acids with sodium hydroxide is constant in value.
(d) Consider the reaction represented by the following equation:
Q\(_{(s)}\) \(\rightleftharpoons\) Q\(_{(l)}\) \(\Delta\) = xkJmol\(^{-1}\)
(i) State with reason which of Q\(_{(s)}\) and O\(_{(J)}\) has the higher entropy.
(ii) What will be the effect of decrease in temperature on the system at equilibrium?
Question 55 Report
(a)(i) State three characteristics of a homologous series.
(ii) Give the name and structural formula of the second member of the alkyne series.
(iii) Write an equation to represent the combustion of ethane in excess oxygen.
(b) Name the type of reaction involved in the conversion of ethanol to
(i) ethene;
(ii) ethylethanoate;
(iii) chloroethane;
(iv) ethoxide
(v) ethanoic acid
(c) Consider the following compound.
(i) Write its IUPAC name.
(ii) Give its molecular formula and empirical formula
(iii) List the products of its H H 0 reaction with saturated Na\(_2\)CO\(_3\) solution.
(iv) State with reason whether its boiling point will be higher or lower than that of the corresponding alkane.
(d) A vegetable oil X was treated with activated charcoal and then with a gas Y in the presence of a catalyst in order to manufacture
(i) Identify Y.
(ii) State the function of the activated charcoal.
(iii) What is the catalyst used?
(iv) If a sample of X is heated with concentrated sodium hydroxide solution, list the products that will be obtained.
Answer Details
None
Question 56 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
All your burette readings (initial and final), as well as the size of your pipette, must be recorded but on no account of experiment procedure is required. All calculations must be done in your answer book.
A is mol dm HCI. B is a solution containing 15.0 g dm of a mixture of NaCl and KHCO\(_3\).
(a) Put A burette and titrate it against 20.0cm\(^3\) or 25.0cm\(^3\) portions of B using methyl orange as indicator. Record the volume of your pipette. Tabulate your burette readings and calculate the average volume of A used. The equation for the reaction involved in the titration is: HCl\(_{aq}\) + KHCO\(_{3(aq)}\) \(\to\) KCl\(_{(aq)}\) +CO\(_{2(g)}\)
(b) From your results and the information provided above, calculate the:
(i) concentration of KHCO\(_3\), in mol dm\(^{-3}\) in B;
(ii) mass of KHCO\(_3\), in g dm\(^{-3}\) in B
(ii) Percentage by mass of KHCO\(_{3}\) in the mixture, [H=1; C = 12; O = 16; K = 39]
(iv) mass of NaCl in the mixture.
Question 57 Report
(a) List two substances that can be used in the laboratory to
(i) dry hydrogen;
(ii) remove carbon (IV) oxide from a sample of air;
(iii) convert hot copper (II) oxide to copper;
(iv) prepare zinc chloride by the action of dilute HCI.
(b)(i) Name two alloys which contain lead.
(ii) State and explain what is observed on bubbling H\(_2\)S into a solution of Pb(NO)\(_2\).
(iii) A metal M exists as a silvery white solid at temperatures above 18°C and as a grey solid below 18°C.
I. name the phenomenon exhibited by M.
II. What term is used to describe the temperature given as 18°C in this case?
(c)(i) Write an equation for the action of heat on each of the following compounds:
I. AgNO\(_3\)
II. (NH4)\(_2\)CO\(_3\).
(ii) Copy and complete the table below
| Metal |
Name of main ore | Method of extraction | One major use Haematite |
| — |
Haematite | — | — |
| — |
— | Electrolysis of molten oxide | — |
Answer Details
None
Question 58 Report
(a)(i) Draw and label a simple cell for the electrolytic purification of copper.
(ii) Write can equation for the reaction at each electrode in (a)(i) above.
(iii) State with reason whether the Daniell cell is an electrolytic cell or an electrochemical cell.
(iv) What is the function of MnO\(_2\) in the Laclanche cell?
(b) Consider the following equation: MnO\(^-_4\) + 8H\(^+\) + xe\(^-\) \(\to\) Mn\(^{2+}\) + yH\(_2\)O. State the
(i) values of x and y;
(ii) oxidation state of Mn in MnO\(^-_4\).
(c)(i) List three factors that affect selective discharge of ions during electrolysis
(ii) State Faraday's second law of electrolysis.
(iii) A voltameter containing silver trioxonitrate(V) solution was connected in series to another voltameter containing copper (II) tetraoxosulphate(VI) solution. When a current ri 0.200 ampere was passed through the solutions, 0.780g of silver was deposited. Calculate the
I. mass of copper that would be deposited in the copper voltameter
II. quantity of electricity used and the time of current flow. [Cu = 63.5 ; Ag = 108; 1F = 96500C]
Question 59 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
Credit will be given for strict adherence to instructions, for observations precisely recorded, and for accurate inferences. All tests, observations, and inferences must be clearly entered in your answer book, in ink, at the time they are made.
C is one of the following substances; starch or sucrose or glucose D is a simple salt. Carry out the following exercises on C and D. Record your observations and identify any gases evolved. State the conclusion you draw from the result of each test.
(a)(i) Add about 5 cm\(^3\) of distilled water to a portion of C in a test tube. Stir thoroughly and test with litmus
(ii) Add about 2cm\(^2\) of Fehling's solution to the resulting mixture from (a)(i) above the heat.
(b)(i) Heat a portion of D strongly in a test tube
(ii) Put the rest of D in a boiling tube and add about 10 cm\(^3\) of distilled water. Shake the mixture
(iii) Put about 2 cm\(^3\) of the mixture from (b)(ii)) in a test tube. Add aqueous ammonia in drops and then in excess
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Question 60 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
(a) If you were provided with anhydrous Na\(_2\)CO\(_3\), spatula and stirrer;
(i) list three other materials you would require to prepare a standard solution of Na\(_2\)CO\(_3\)
(ii) state what you would observe on adding diluted H\(_2\)SO\(_4\) to a portion of the Na\(_2\)CO\(_3\)
(b)(i) Describe briefly one chemical test you would perform to distinguish between zinc ions and aluminium ions in solution.
(ii) Mention one laboratory reagent you would use to;
I. produce ammonia from (NH\(_4\))\(_2\)SO\(_4\)
II. differentiate between precipitates of AgCl and Agl
lll. dehydrate ethanol
(c) Give the reason for each of the following laboratory practices
(i) Aqueous solutions of FeSO\(_4\) are freshly prepared when required for use.
(ii) The first jar of hydrogen collected during its preparation is discarded
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Question 61 Report
(a) Describe briefly a suitable procedure for preparing a pure sample of MgSO\(_4\) starting from MgO.
(b)(i) Mention two sources of water pollution.
(ii) Explain why the sample of air collected in the process of boiling water is richer in oxygen than atmospheric air
(iii) Mention one substance used as coagulant in water treatment plants.
(c)(i) State two physical porperties of chlorine.
(ii) Write an equation to show how chlorine reacts with iron
(iii) Why is Chlorine preferred to sulphur (IV) oxide in the bleaching of cotton
(d) Bleaching powder reacts with dilute HCl according to the reaction below;
CaOCl\(_{2(s)}\) + 2HCI\(_{(aq)}\) -> CaCl\(_{2(aq)}\) + H\(_2\)O\(_{(l)}\) + Cl\(_{2(g)}\)
Calculate the mass of bleaching powder that will produce 400cm\(^3\) of chlorine at 25\(^o\)C and a pressure of 1.20 x 10\(^5\) NM\(^{-2}\). [O = 16.0; Cl = 35.5; Ca = 40.0;1 mole of gas occupies 22.4 dm\(^3\) at s.t.p; standard pressure = 1.01 x 10\(^6\) Nm\(^{-2}\)]
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