WAEC SSCE - Chemistry - 1991
Question 1 Report
In which of the following is the oxidation number of nitrogen zero?
Answer Details
The oxidation number of an element is defined as the charge that it would carry if all the shared electrons are assigned to the more electronegative atom. The sum of the oxidation numbers of all atoms in a molecule must be equal to the charge of the molecule. In NH3, the oxidation number of nitrogen is -3 because hydrogen has an oxidation number of +1 and the sum of oxidation numbers in the compound is zero. In NaNO3, the oxidation number of nitrogen is +5 because sodium has an oxidation number of +1 and oxygen has an oxidation number of -2. In HNO2, the oxidation number of nitrogen is +3 because hydrogen has an oxidation number of +1 and oxygen has an oxidation number of -2. In NOI3, the oxidation number of nitrogen is +5 because oxygen has an oxidation number of -2 and iodine has an oxidation number of +7. The only option where nitrogen has an oxidation number of zero is N2, because it is a diatomic molecule and the oxidation number of each nitrogen atom is zero.
Question 2 Report
When starch undergoes complete enzyme-catalyzed hydrolysis, the resulting product is
Answer Details
When starch undergoes complete enzyme-catalyzed hydrolysis, it is broken down into its constituent glucose molecules. Starch is a polymer made up of glucose units, and enzymes such as amylase and amyloglucosidase can break the glycosidic bonds between these units, resulting in the formation of individual glucose molecules. Therefore, the resulting product of complete enzyme-catalyzed hydrolysis of starch is glucose.
Question 3 Report
A current of 4.0 amperes was passed through copper (ll) tetraoxosulphate (IV) solution for one hour using copper electrodes. What was the mass of copper deposited? (Cu = 64, 1F = 96500 C)
Answer Details
Question 4 Report
Which of the processes represented by the following equations has the greatest positive entropy change?
Answer Details
Entropy is a measure of the degree of randomness or disorder in a system. The greater the number of ways in which the particles in a system can be arranged, the greater the entropy of that system. The process that has the greatest positive entropy change is the one that involves the largest increase in the degree of randomness or disorder of the particles. This occurs when a solid or liquid is converted to a gas or when a gas is allowed to expand into a larger volume. Looking at the given equations, we can see that the equation (a) C6H3(l) → C6H 6 (g) involves the conversion of a liquid to a gas, which leads to a large increase in the number of ways in which the particles can be arranged. Therefore, this process has the greatest positive entropy change among the given equations. Note: The answer may vary depending on the reference state and conditions under which the reactions occur.
Question 5 Report
In which of the following are the substances arranged in their correct order of increasing melting point?
Answer Details
Question 6 Report
In the redox reaction represented by the following equation: Cu2+aq + Zn(s) → Cu(s) + Zn2+
Answer Details
In the given redox reaction, the copper (ll) ions (Cu2+) are being reduced to copper atoms (Cu) while the zinc atoms (Zn) are being oxidized to zinc ions (Zn2+). Therefore, "copper (ll) ions are reduced to copper atoms" is correct.
Question 7 Report
CH2 = CH2 + H2SO4 → CH3 - CH2 -OSO3H. The reaction illustrated by the equation above is an example of
Answer Details
The reaction illustrated in the equation above is an example of an addition reaction. Addition reactions are a type of organic reaction where two or more molecules combine to form a larger molecule with no elimination of any atoms. In this case, the double bond in ethene (CH2=CH2) reacts with the sulfuric acid (H2SO4) to form a single bond between carbon atoms, resulting in the formation of ethyl hydrogen sulfate (CH3-CH2-OSO3H).
Question 8 Report
Esterification of propane 1,2,3-triol and unsaturated higher carboxylic acids will produce
Question 9 Report
Which of the following modes of motion is exhibited by the particles of a solid?
Answer Details
The particles of a solid exhibit vibrational motion only. A solid is one of the three states of matter, in which the particles are closely packed together and have a fixed shape and volume. The particles of a solid are not free to move around like those in a liquid or gas. Instead, they can only vibrate around their fixed positions. Therefore, the only mode of motion exhibited by the particles of a solid is vibrational motion, which means that the particles oscillate back and forth around their fixed positions. They do not move from one place to another, which is referred to as translational motion, nor do they move randomly, which is referred to as random motion.
Question 10 Report
2NaNO3 → 2NaNO2 + O2. From the equation above, what is the volume of oxygen produced at s.t.p. when 8.5g of 2NaNO3 is heated until no further gas is evolved? (2NaNO3 = 85, molar volume of gases at s.t.p. = 22.4dm3)
Answer Details
The balanced chemical equation is 2NaNO3 → 2NaNO2 + O2. It shows that 2 moles of NaNO3 produces 1 mole of O2. We are given 8.5g of 2NaNO3. To find the number of moles, we divide the mass by the molar mass. Molar mass of 2NaNO3 = (2 x 23) + 2(14 + 3x16) = 46 + 2(14 + 48) = 46 + 124 = 170g/mol. Number of moles of 2NaNO3 = 8.5g / 170g/mol = 0.05mol. Since 2 moles of NaNO3 produces 1 mole of O2, the number of moles of O2 produced is also 0.05mol. The molar volume of gases at s.t.p. is 22.4dm3/mol. Therefore, the volume of O2 produced at s.t.p. is: Volume of O2 = Number of moles x Molar volume of gases at s.t.p. = 0.05mol x 22.4dm3/mol = 1.12dm3 Therefore, the volume of oxygen produced at s.t.p. when 8.5g of 2NaNO3 is heated until no further gas is evolved is 1.12dm3. Hence, the correct option is 1.12dm3.
Question 11 Report
In which of the following crystals are the particles held by van der Waal's forces only?
Answer Details
Van der Waal's forces are weak intermolecular forces that exist between molecules. These forces are formed due to the attraction between the temporary dipoles that arise due to the fluctuations in the electron cloud of molecules. Out of the given options, only iodine is held together by van der Waal's forces only. Iodine exists as a diatomic molecule, and each iodine atom is held together by a covalent bond. However, the molecules are held together in the crystal lattice by weak van der Waal's forces. Sodium chloride, ice, diamond, and quartz are all held together by strong ionic or covalent bonds, and therefore, van der Waal's forces are not the primary forces holding these crystals together.
Question 12 Report
What is the amount (in mole) of sodium trioxocarbonate (IV) in 5.3 g of the compound? (Na2CO3 = 106)
Answer Details
The molar mass of sodium trioxocarbonate (IV) is 2(23) + 12 + 3(16) = 106 g/mol (by adding the atomic masses of the elements present in one mole of the compound). To find the amount (in moles) of the compound in 5.3 g, we need to divide the given mass by the molar mass: Amount of Na2CO3 = Mass of Na2CO3 / Molar mass of Na2CO3 Amount of Na2CO3 = 5.3 g / 106 g/mol Amount of Na2CO3 = 0.05 mol Therefore, the amount (in moles) of sodium trioxocarbonate (IV) in 5.3 g of the compound is 0.05. The answer is.
Question 13 Report
Which of the following is suitable for determining different isotopes present in an element which exhibits isotopy?
Answer Details
Mass spectrometer is suitable for determining different isotopes present in an element which exhibits isotopy. This is because mass spectrometer can separate different isotopes based on their mass-to-charge ratio. In a mass spectrometer, the sample is ionized and then accelerated in an electric field. The ions are then separated based on their mass-to-charge ratio using a magnetic field. The detector records the number of ions of each mass-to-charge ratio, which can be used to determine the relative abundance of each isotope present in the sample. Therefore, mass spectrometer is a very useful tool in the study of isotopes and can be used to identify and quantify different isotopes in a sample.
Question 14 Report
The separation of a mixture of calcium trioxocarbonate (lV) and sodium trioxocarbonate (IV) is most easily carried out by using the differences in their
Answer Details
The separation of a mixture of calcium trioxocarbonate (lV) and sodium trioxocarbonate (IV) is most easily carried out by using the differences in their solubility. When two or more substances are mixed together, they may have different solubility in a particular solvent. In this case, calcium trioxocarbonate (IV) and sodium trioxocarbonate (IV) are both soluble in water, but their solubility is different. Calcium trioxocarbonate (IV) is less soluble in water compared to sodium trioxocarbonate (IV). Therefore, by dissolving the mixture in water, the less soluble calcium trioxocarbonate (IV) can be separated from the more soluble sodium trioxocarbonate (IV) by filtration or centrifugation. This method is called fractional crystallization.
Question 15 Report
Which of the following statements is not correct? Group 7 elements
Answer Details
The statement that is not correct about Group 7 elements is: "have relatively low ionization potentials." Explanation: Group 7 elements, also known as halogens, include fluorine, chlorine, bromine, iodine, and astatine. These elements are diatomic, meaning that they exist naturally as a molecule containing two atoms of the same element. They are highly electronegative, which means that they have a strong attraction for electrons. This high electronegativity makes them good oxidizing agents since they readily accept electrons from other atoms. However, the statement that Group 7 elements have relatively low ionization potentials is incorrect. Ionization potential refers to the amount of energy required to remove an electron from an atom or ion. Halogens have relatively high ionization potentials since they have a strong attraction for their outermost electrons. This means that it takes a significant amount of energy to remove an electron from a halogen atom or ion, making it less likely to form a cation. Therefore, the correct answer is "have relatively low ionization potentials."
Question 16 Report
An organic compound which reacts readily with bromine to form a compound with the formula CH3CHBrCH2Br is
Answer Details
The organic compound which reacts readily with bromine to form a compound with the formula CH3CHBrCH2Br is propene. Propene is an unsaturated hydrocarbon with the chemical formula C3H6. It contains a carbon-carbon double bond that is readily attacked by bromine in the presence of an appropriate catalyst. The addition of two bromine atoms across the double bond of propene produces 2-bromopropane, which has the formula CH3CHBrCH2Br. This reaction is an example of electrophilic addition, in which an electrophile (in this case, Br2) is added to an unsaturated molecule (propene) to form a saturated molecule (2-bromopropane). Therefore, propene is the organic compound that reacts readily with bromine to form 2-bromopropane.
Question 17 Report
Which of the reactions represented by the following equations will take place at room temperature?
Answer Details
The reaction that will take place at room temperature is (2Na + 2H2O → 2NaOH + H2). This is because sodium is a highly reactive metal and it readily reacts with water at room temperature to form sodium hydroxide and hydrogen gas. The other reactions require higher temperatures or catalysts for the reactions to occur.
Question 18 Report
When air is passed through a heated tube containing finely divided copper, the component that is absorbed in the process is
Answer Details
When air is passed through a heated tube containing finely divided copper, oxygen is the component that is absorbed in the process. This is because copper is a good catalyst for the oxidation of gases, especially oxygen. As air passes through the heated tube containing finely divided copper, the copper catalyses the oxidation of oxygen in the air to form copper oxide. The copper oxide is then absorbed onto the surface of the copper, leaving behind the other components of the air, such as nitrogen, carbon dioxide, water vapour, and noble gases. Therefore, the correct option is oxygen.
Question 19 Report
The ratio of reactants to products is 1: 3: 2 in the reaction represented by the equation below: N2,/SUB> (g) → 2NH3(g) which of the following law is demonstrated by this?
Question 20 Report
Which of the following formula is that of a dicarboxylic acid?
Answer Details
The formula of a dicarboxylic acid is a molecule with two carboxylic acid functional groups (-COOH) present in its structure. The correct option is (d) CH2(COOH)2, which is the formula for oxalic acid, a dicarboxylic acid commonly found in plants and used in industrial applications such as rust removal and bleaching.
Question 21 Report
A compound which liberates carbon (IV) oxide from a hydrogentrioxocarbonate (lV) could have the molecular formula
Answer Details
The compound which liberates carbon (IV) oxide from a hydrogen trioxocarbonate (IV) is an acid. The molecular formula of an acid is usually expressed as HX, where X is the anion of the acid. Therefore, the molecular formula of the compound could be HCOOH (formic acid). When formic acid is added to hydrogen trioxocarbonate (IV), it reacts to liberate carbon (IV) oxide gas, as shown by the following equation: 2HCOOH + H2CO3 → 2H2O + 2CO2 Therefore, formic acid is a possible compound that could liberate carbon (IV) oxide from a hydrogen trioxocarbonate (IV).
Question 22 Report
In solution, aminoethanoic acid (glycine) can be represented as NH+3 CH2COO. This implies that it
Answer Details
The representation of aminoethanoic acid (glycine) as NH+3 CH2COO indicates that it can function as a weak acid or a weak base. The NH+3 group is a positively charged ion (cation) which can act as an acid by donating a hydrogen ion (proton) to a base. On the other hand, the CH2COO group is a negatively charged ion (anion) which can act as a base by accepting a proton from an acid. Therefore, aminoethanoic acid (glycine) can function as both an acid and a base in solution, depending on the nature of the other species present in the solution.
Question 23 Report
The metal extracted from cassiterite is
Answer Details
The metal extracted from cassiterite is tin. Cassiterite is a mineral composed of tin dioxide (SnO2), and it is the primary ore of tin. Tin is a silvery-white metal that is commonly used to coat other metals to prevent corrosion. It is also used to make alloys, such as bronze and pewter, and is an important component of solders. Tin has a low toxicity, which makes it suitable for use in food packaging and other applications where contact with humans or animals is possible.
Question 24 Report
Brass is an alloy of copper and
Answer Details
Brass is an alloy of copper and zinc. An alloy is a combination of two or more metals, or a metal and a non-metal. In the case of brass, copper is the main metal and zinc is the other component. The proportion of copper to zinc can vary, resulting in different types of brass with varying properties. Brass is known for its attractive golden appearance and is widely used in the production of decorative items, musical instruments, and plumbing fixtures, among other things.
Question 26 Report
Compounds that have the same molecular formula but different structures are said to be
Answer Details
Compounds that have the same molecular formula but different structures are said to be isomeric. Isomers are molecules that have the same number and types of atoms but different arrangements of those atoms. This means that they have different physical and chemical properties, even though they have the same molecular formula. For example, butane and isobutane both have the molecular formula C4H10, but they have different structures and therefore different properties. This property of compounds to have same molecular formula but different structures is called isomerism.
Question 27 Report
Which of the following properties is not characteristic of electrovalent compounds?
Answer Details
The property that is not characteristic of electrovalent compounds is "high vapour pressures". Electrovalent compounds, also known as ionic compounds, have high melting and boiling points due to the strong electrostatic forces of attraction between oppositely charged ions in the crystal lattice. They also tend to form crystalline solids and are typically soluble in polar solvents. In addition, electrovalent compounds can conduct electricity in aqueous solution because the ions are free to move and carry an electric charge. However, they do not have high vapour pressures because they are held together by strong ionic bonds and are not easily vaporized.
Question 28 Report
CH4(g) + 2O2(g) → 2H2O(l) + CO2(g) ∆H = 890KJ mo-1 ∆H in the reaction represented by the equation above is the enthalpy of
Answer Details
The ∆H in the given chemical equation refers to the enthalpy change or heat change of the reaction. It is the difference between the enthalpy of the products and the enthalpy of the reactants. In this equation, energy is released in the form of heat (exothermic reaction), and the value of ∆H is 890KJ mo-1. Since the reactants in the equation include CH4 and O2, which are the typical fuels used in combustion reactions, it can be concluded that the reaction is a combustion reaction. Therefore, the correct answer is "combustion".
Question 29 Report
The products of the electrolysis of dilute sodium chlorid solution with platinum electrodes are
Answer Details
Question 30 Report
Which of the following is not a direct petroleum product?
Answer Details
Methane, Ethanol, Petrol, Kerosene are all direct petroleum products as they are obtained directly from the refining of crude oil. Vaseline, on the other hand, is not a direct petroleum product. It is produced from petroleum jelly, which is a semi-solid mixture of hydrocarbons obtained from petroleum. Vaseline is obtained from petroleum jelly through a refining process that removes impurities and increases its purity. Thus, Vaseline is a derivative of petroleum, but not a direct petroleum product.
Question 31 Report
Which of the following elements can from more than one acidic oxide?
Answer Details
Question 32 Report
Consider the reaction represented by the equation below: H2(g) + 12(s) ⇌ 2HI(g) ∆H negative. Which of the following takes place when the temperature of the reaction vessel is decreased?
Answer Details
When the temperature of the reaction vessel is decreased, the equilibrium shifts to favor the exothermic direction, which is the forward reaction in this case. As a result, more hydrogen and iodine molecules react to form hydrogen iodide. The equilibrium constant (K) for this reaction indicates that the reaction favors the products, which means that at equilibrium, there is a greater concentration of hydrogen iodide molecules than hydrogen and iodine molecules. Therefore, a decrease in temperature will increase the yield of hydrogen iodide molecules, resulting in a shift towards the forward reaction. Therefore, the correct option is "the yield of hydrogen iodide increases".
Question 33 Report
When a crystal was added to its solution, it did not dissolve and the solution remained unchanged, showing that the solution was
Answer Details
The solution is saturated. A saturated solution is a solution that contains the maximum amount of solute that can be dissolved in the solvent at a given temperature and pressure. When a crystal is added to a saturated solution, it will not dissolve because there is no more room for additional solute to dissolve. The solution remains unchanged because the concentration of solute in the solution is already at its maximum limit, and no more solute can be dissolved.
Question 34 Report
Hydrogen is used for the following except
Answer Details
Hydrogen is used for all of the following except extinguishing fire. Hydrogen gas itself is highly flammable and can even ignite explosively in the presence of air, oxygen or any other oxidizing gas. It does not work as an extinguisher and, in fact, can even make a fire worse by adding fuel to the fire. The other options listed are all valid uses of hydrogen. It is used in the manufacturing of ammonia, the synthesis of hydrochloric acid, the conversion of coal to petrol and in the manufacture of margarine.
Question 35 Report
How many principal electronic shells has an atom whose electronic configuration is shown below? 1s22s22p63s1
Answer Details
The electronic configuration of an atom shows the distribution of electrons in its various energy levels or shells. Each shell can hold a certain number of electrons. The first shell can hold up to two electrons, the second shell can hold up to eight electrons, and the third shell can hold up to 18 electrons. The electronic configuration given as 1s22s22p63s1 shows that there are electrons in the first, second, and third shells. The first shell has two electrons (1s2), the second shell has eight electrons (2s22p6), and the third shell has one electron (3s1). Therefore, the atom has three principal electronic shells. Answer: 3.
Question 36 Report
A colourless and odourless gas X burns in oxygen with a pale blue flame.
(a) Suggest two gases which X could be.
(b) Give one chemical test that could be used to confirm which of the two gases X is.
Answer Details
None
Question 37 Report
The set-up shown in the diagram below was used to separate a drop of universal indicator into the constituent dyes using ethyl ethanoate as the solvent.
(a) What name is given to the separate strated in the diagram?
(b) State: (i) how many components are resolved in the separation;
(ii) the material normally used in laborary as the adsorbent medium;
(iii) which of the labels the point of application of the indicator.
None
Answer Details
None
Question 38 Report
(a) State two factors which can affect the rate of a chemical reaction.
(b) 0.72g of magnesium was added to different volumes of 2 mol. per dm\(^3\) hydrochloric acid. The volume of liberated was as measured at room temperature and pressure. The result of the experiment was as tabulated
| vol. of 2 mol. per dm\(^3\) HCl used (cm\(^3\) | Vol. of H\(_2\) evolved in cm\(^3\) (to the nearest 10cm\(^3\)) |
| 5 15 25 35 45 |
120 360 550 600 600 |
Use the data in the table to plot a graph of the volume of hydrogen liberated against the volume of acid used.
(c) From the graph in (b) above, determine the volume of: (i) hydrogen that would be produced if 50 cm\(^3\) of the acid were added to 0.72g of magnesium.
(ii) the acid which must be added to 0.72 g of magnesium to produce 480 cm\(^3\) of hydrogen;
(iii) the acid needed exactly to dissolve 0.72 g of magnesium completely.
(d) Explain your answer to (c)(iii).
(e) From your answers to (c) above, deduce the: (i) volume of the acid which will dissolve 1 mole of magnesium completely. (Mg = 24)
(ii) volume of hydrogen that would be liberated if 1 mole of magnesium dissolves completely in the acid;
(iii) equation for the reaction between magnesium and hydrochloric acid. Show clearly how you arrived at you answers
Question 39 Report
(a)State three characteristics of a catalyst.
(b) Mention one manufacturing process in which each of the following metals is used as a catalyst:
(i) iron;
(ii) nickel;
(iii) platinum
(c) Give one example of an organic catalyst.
Answer Details
None
Question 40 Report
(a) Give two reasons why fused alumina is mixed with cryolite in the electrolytic extraction of aluminium.
(b) Write an equation for the reaction of sodium hydroxide with bauxite.
Answer Details
None
Question 41 Report
Give one oxide in each case which;
(a) can act as a reducing agent
(b) can be used as a refrigerant
(c) is the anhydride of a strong acid;
(d) is yellow when hot and white then hot and white when cold;
(f) is usad as a pigment in paints.
Answer Details
None
Question 42 Report
Methane is obtained when a powdered mixture of anhydrous sodium ethanoate and soda-lime is heated in a hard glass test tube.
(a) Write an equation for the reaction.
b) Explain briefly why soda-lime is preferred to sodium hydroxide for the preparation.
Answer Details
None
Question 43 Report
(a) Name the industrial process by which ethene is obtained from petroleum fractions
(b) Give the I. U. P.A.C name of the isomer whose structure is shown below.
(c) Illustrate with an equation, one reaction in which benzene behaves as:
(i) unsaturated hydrocarbon
(ii) a saturated hydrocarbon
Answer Details
None
Question 44 Report
(a)(i) Give two uses of chlorine.
(ii) State the action of chlorine on moist blue litmus paper
(b) Draw a labelled diagram for the laboratory preparation of a dry sample of chlorine
(c) State the type of reaction involved between chlorine and (i) aqueous iron (II) chloride;
(ii) propane. Write an equation for each reaction and name the product formed in (c)(ii).
(d) Consider the reactions the following equations: Cl\(_{2(g)}\) + 2Br\(^-_{(aq)}\) \(\to\) 2Cl\(^-_{(aq)}\) + Br\(_{2(g)}\)
F\(_{2(g)}\) + 2Cl\(^-_{(aq)}\) ---> 2F\(^-_{(aq)}\) + Cl\(_{2(g)}\)
From the equations, arrange bromine, chlorine and fluorine in increasing order of oxidizing ability. Give the reason for your answer.
Question 45 Report
(a) Give three differences between electrovalent compounds and covalent compounds
(b) List two physical properties of metals which can be accounted for by their structure
(c) Thorium (Th) metal undergoes a reaction represented by the following equation:
\(^{234}_{90}Th \to X + ^{234}_{91}Pa\)
(i) State the type of process involved in the reaction
(ii) Balance the equation equation and hence identify X.
(iii) Name one equipment which can be used to detect X.
(iv) Sketch a curveto show the mass of given quantity of thorium will change over a long period of time.
(d) Y is a moderately reactive divalent found naturally in the combined state as the trioxocarbonate (IV) salt, YCO\(_3\) is decomposed by strong heat, state the steps you would use in extracting Y from the ore. Write equation to show the chemical processes involved.
Question 46 Report
Sketch a curve to show how the solubility of a gas varies with increasing temperature
Answer Details
None
Question 47 Report
State the atoms represented as shown below:
(a) State the relationship between the two atoms.
(b) What is the difference between them?
(c) Give two examples of elements which exhibit the phenomenon illustrated above.
Question 48 Report
(a) Name one gaseous hydrocarbon which is
(i) used for welding.
(ii) a major raw material for the plastic industry.
(b) Write the structural formula of the hydrocarbon in (a)(i) above. Name the process by which it can be converted to neoprene rubber.
(c) Potatoes contain a high proportion of carbohydrate.
(i) Give the main product formed when potatoes are dehydrated completely
(ii) Describe how you would convert potatoes to ethanol. State the reactions involved the process and write equation for the final stage of the conversion.
(iii) Draw a labelled diagram of the apparatus you would use to obtain a sample of fairly pure ethanol from the product formed in (c)(ii) above. What is the name given to the technique?
Answer Details
None
Question 49 Report
(a) Give the products of electrolysis of dilute copper (II) tetraoxosulphate(VI) solution using the following materials as electrodes:
(i) carbon rod;
(ii) copper rods
(b) For each of the process in (a) above;
(i) write the anodic half reaction;
(ii) state how electrolysis affects the pH of electrolyte
