WAEC SSCE - Chemistry - 1994
Question 1 Report
What is the molar mass of an alkyne with the formula Cx H 14? (H = 1, C = 12)
Answer Details
Question 2 Report
Tetraoxosulphate (lV) acid is described as strong acid because it is highly
Answer Details
Tetraoxosulphate (IV) acid, also known as sulfuric acid, is considered a strong acid because it completely ionizes in water. When sulfuric acid dissolves in water, it breaks down completely into hydrogen ions (H+) and sulfate ions (SO4^2-). This means that all the sulfuric acid molecules present in the solution donate their hydrogen ions to the water, resulting in a high concentration of H+ ions in the solution. These H+ ions can react with other substances, making sulfuric acid a powerful and reactive acid. Therefore, - "ionized in water" - is the correct answer.
Question 3 Report
In a chemical reaction, the reacting species possess energy of motion known as
Answer Details
The energy of motion possessed by the reacting species in a chemical reaction is known as kinetic energy. Kinetic energy is the energy of motion. When a substance is in motion, it possesses kinetic energy. In a chemical reaction, the reactants are in motion and collide with each other, causing the chemical reaction to occur. This motion is due to the kinetic energy of the particles. The kinetic energy of the particles in a substance depends on its temperature. As the temperature of a substance increases, the kinetic energy of the particles also increases, causing them to move faster and collide more frequently. This, in turn, increases the rate of the chemical reaction. Therefore, the reacting species in a chemical reaction possess kinetic energy, which is the energy of motion.
Question 5 Report
Which of the following occurs when an aqueous solution of sodium hydroxide is electrolysed using graphite electrodes?
Answer Details
When an aqueous solution of sodium hydroxide (NaOH) is electrolyzed using graphite electrodes, the following occurs: At the cathode (negative electrode), hydrogen gas is produced through the reduction of water molecules. This is because water has a lower reduction potential than Na+ ions in the solution. 2H2O(l) + 2e- -> H2(g) + 2OH-(aq) At the anode (positive electrode), the hydroxide ions (OH-) are oxidized to form oxygen gas and water molecules. This is because OH- ions have a higher oxidation potential than water molecules. 4OH-(aq) -> 2H2O(l) + O2(g) + 4e- Therefore, the correct option is (c) Oxygen gas is produced at the anode.
Question 6 Report
The number of atoms in 1.2g of carbon - 12 isotope is
Answer Details
The first step to solving this problem is to determine the number of moles of carbon-12 present in 1.2g of the isotope. We do this by dividing the mass of the isotope by its molar mass. The molar mass of carbon-12 is 12 g/mol. Number of moles of carbon-12 = 1.2 g / 12 g/mol = 0.1 mol Since each mole of carbon-12 contains Avogadro's number of atoms (6.02 x 10^23), we can determine the number of atoms in 0.1 mol of carbon-12 as: Number of atoms = 0.1 mol x 6.02 x 10^23 atoms/mol = 6.02 x 10^22 atoms Therefore, the answer is 6.02 x 10^22.
Question 9 Report
Sodium chloride is used in the following processes except in the
Question 10 Report
Catalytic hydrogenation of alkenes produces compounds with the general formula
Answer Details
The correct answer is (c) CnH2n+2. When alkenes undergo catalytic hydrogenation, each double bond in the molecule is converted into a single bond, and two hydrogen atoms are added to the molecule. This process is a type of addition reaction, and the general formula of the resulting compounds is CnH2n+2. Therefore, is the correct answer.
Question 11 Report
How many faradays of electricity are required to liberate 9g aluminium? (AI = 27)
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Question 12 Report
When water is dropped on calcium carbide, the gaseous product is an
Answer Details
When water is dropped on calcium carbide, the gaseous product formed is acetylene (C2H2), which is an alkyne. Calcium carbide (CaC2) reacts with water (H2O) to produce acetylene gas and calcium hydroxide (Ca(OH)2) according to the following equation: CaC2 + 2H2O → C2H2 + Ca(OH)2 Acetylene gas is a colorless, highly flammable gas with a distinctive odor. It is commonly used in welding and cutting torches, as well as in the production of various organic chemicals.
Question 13 Report
Which of the following is likely to have the highest degree of hardness?
Answer Details
Question 14 Report
Study the reaction represented by the equation: Alkanol + Alkanoic acid conc. H2SO4 Alkanoate + water. The type of process involved in the reverse reaction is
Answer Details
The type of process involved in the reverse reaction is hydrolysis. Hydrolysis is a chemical reaction in which water is used to break down a compound. In the given reaction, an alkanol and an alkanoic acid react in the presence of concentrated sulfuric acid to form an alkanoate and water. The reverse reaction involves the breakdown of the alkanoate using water to form the alkanol and alkanoic acid. This process is called hydrolysis.
Question 15 Report
The positive of an element in the Periodic Table is determined by
Answer Details
The positive charge of an element in the Periodic Table is determined by the number of protons in its atom. This is because the positive charge of an atom is equal to the number of protons in its nucleus, which is also known as its atomic number. The atomic number is the defining characteristic of an element and determines its position in the Periodic Table. Each element has a unique atomic number which corresponds to the number of protons in its nucleus. Therefore, the number of protons in an atom determines its positive charge and its position in the Periodic Table.
Question 16 Report
The following compounds contain the same type of bonds except
Answer Details
The compound that does not contain the same type of bonds as the others is hydrogen chloride. Hydrogen chloride is a covalent compound, while the others are all ionic compounds. Covalent bonds are formed by the sharing of electrons between atoms, while ionic bonds are formed by the transfer of electrons from one atom to another. In hydrogen chloride, the hydrogen atom and chlorine atom share electrons to form a covalent bond. In contrast, in sodium chloride, magnesium chloride, potassium chloride, and lithium chloride, the metal atom donates electrons to the nonmetal atom to form an ionic bond. Therefore, all the other compounds contain ionic bonds, while hydrogen chloride contains a covalent bond.
Question 17 Report
Which of the following reactions is accompanied by the first ionization energy of an element X?
Answer Details
Question 18 Report
The oxidation number of phosphorus in PO 3/4 is
Answer Details
The oxidation number of phosphorus in PO3/4 is +5. To determine the oxidation number of phosphorus, we can use the fact that the sum of the oxidation numbers of all atoms in a neutral compound is zero. Since oxygen has an oxidation number of -2, we can set up the equation: x + 4(-2) = 0 where x is the oxidation number of phosphorus. Solving for x gives: x = +5 Therefore, the oxidation number of phosphorus in PO3/4 is +5.
Question 19 Report
Alkanols have unexpectedly high boiling points relative to their molar masses because of intermolecular
Answer Details
Alkanols, also known as alcohols, have unexpectedly high boiling points relative to their molar masses because of intermolecular hydrogen bonding. Hydrogen bonding is a type of intermolecular force that occurs when a hydrogen atom bonded to an electronegative atom, such as oxygen or nitrogen, is attracted to another electronegative atom in a nearby molecule. In the case of alkanols, the hydrogen atom attached to the oxygen atom in one molecule can form a hydrogen bond with the oxygen atom of another molecule. This results in a network of intermolecular hydrogen bonds that are much stronger than the weak van der Waals' forces that exist between non-polar molecules of similar size and shape. Due to the presence of these strong intermolecular forces, more thermal energy is required to overcome these forces and cause the molecules to separate, resulting in higher boiling points of alkanols relative to other organic compounds of similar molar mass.
Question 20 Report
Which of the following electronic structures belongs to a noble gas?
Answer Details
The electronic structure of a noble gas has a completely filled outermost shell. Among the options, only 1s22s22p63s23p6, has a completely filled outermost shell. This electronic configuration corresponds to the noble gas argon (Ar). Therefore, is the correct answer.
Question 21 Report
The following will decolourize acidified potassium tetraoxomanganate (VII) solution except
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Question 22 Report
Mg2 + 2HCI(aq) → MgCI2(g) + H2(g) From the equation above what mass of hydrogen would be produced if 12.0 g of magnesium reacted completely with dilute hydrochloric acid? (H = 1, Mg = 24)
Answer Details
Question 23 Report
Which of the following is not a property of magnesium oxide?
Answer Details
The property of magnesium oxide that is not correct is "low binding energy." Magnesium oxide is an ionic compound made up of magnesium and oxygen ions. It has a high melting point and possesses a crystal lattice structure due to the presence of ionic bonds between the ions. Magnesium oxide is also known to dissolve in polar solvents, such as water, due to its ionic nature. However, it is not known for having low binding energy, as it has a strong ionic bond between the magnesium and oxygen ions. Therefore, the property of magnesium oxide that is not correct is "low binding energy."
Question 25 Report
When naphthalene on heating changes from the solid state directly to the gaseous state it undergoes
Answer Details
When naphthalene changes from the solid state directly to the gaseous state upon heating, it undergoes sublimation. Sublimation is the process in which a solid directly changes into a gas without going through the liquid state. This occurs when the vapor pressure of the solid is greater than the atmospheric pressure. In the case of naphthalene, it has a high vapor pressure at room temperature and atmospheric pressure, which allows it to undergo sublimation when heated.
Question 26 Report
Which of the following is not a halogen?
Answer Details
Halogens are a group of chemical elements that include fluorine, chlorine, bromine, iodine, and astatine. These elements share similar chemical properties and can form salts with metals. Silicon, on the other hand, is not a halogen. It is a metalloid element that is commonly found in the Earth's crust. Therefore, is the correct answer as silicon is not a halogen.
Question 27 Report
Which of the following would increase the rate of reaction of chips of a metal M as shown in the equation below? M(s) + 2HCI(aq) → MCI2(aq) + H2(g)
Answer Details
Grinding the metal into powder would increase the rate of reaction of chips of a metal M in the given equation. The rate of reaction depends on the surface area of the reactants in contact with each other. When the metal is in the form of chips, the surface area in contact with the hydrochloric acid is relatively small, and the rate of reaction is slow. However, by grinding the metal into powder, the surface area of the metal in contact with the acid increases significantly, allowing more metal to react at a faster rate. Therefore, grinding the metal into powder increases the rate of reaction. The other options would not increase the rate of reaction of chips of a metal M in the given equation. Diluting the hydrochloric acid or adding distilled water would decrease the concentration of the acid, which would slow down the reaction rate. Decreasing the temperature would decrease the kinetic energy of the molecules, leading to a slower rate of reaction. Increasing the pressure would not have a significant effect on the rate of the reaction in this case.
Question 28 Report
A measure of the degree of disorder in a chemical system is known as the
Answer Details
The measure of the degree of disorder or randomness in a chemical system is known as entropy. Entropy is a thermodynamic quantity that describes the number of ways in which the energy of a system can be distributed among its particles. In simpler terms, it is a measure of how much the energy of a system is spread out or dispersed. The greater the entropy of a system, the more disordered or random it is. Entropy is usually denoted by the symbol S and has units of joules per kelvin (J/K).
Question 29 Report
In any chemical reaction, the total mass of the products is always equal to that of the reactants. This is statement of the law of
Answer Details
The statement "In any chemical reaction, the total mass of the products is always equal to that of the reactants" is the statement of the law of conservation of matter. This law, also known as the law of conservation of mass, states that in a closed system, the total mass of the system remains constant during a chemical reaction. This means that the mass of the reactants before the reaction is the same as the mass of the products after the reaction. In other words, matter cannot be created or destroyed in a chemical reaction; it can only be transformed from one form to another. This law is a fundamental principle of chemistry and is essential in understanding the behavior of matter in chemical reactions. It was first proposed by Antoine Lavoisier, a French chemist in the late 18th century, and has since become one of the most important principles in chemistry.
Question 30 Report
What is the molar of hydrogen sulphide gas in the reaction H2SO4(aq) + 3H2S(g) → 4S(s) + 4H2O (l)n represented by the following equation?
Answer Details
The question doesn't provide options to choose from, but based on the given equation, hydrogen sulfide (H2S) is a reducing agent. A reducing agent is a substance that causes another substance to be reduced by donating electrons to it. In the given equation, hydrogen sulfide (H2S) is donating electrons to sulfuric acid (H2SO4), which causes sulfuric acid to be reduced, and hydrogen sulfide is oxidized in the process. Therefore, hydrogen sulfide is a reducing agent in the given equation.
Question 31 Report
The gaseous product formed when ammonia is passed over heated copper (ll) oxide is
Question 32 Report
If the volume of a given mass of gas at 0oC is 27.3cm3, what will be the volume of the gas at 10oC, pressure remaining constant?
Answer Details
The volume of a gas is directly proportional to its temperature, provided the pressure and the amount of gas remain constant. This relationship is known as Charles's law. According to Charles's law, when the temperature of a gas is increased, its volume will also increase, and when the temperature of a gas is decreased, its volume will also decrease. In this case, the initial volume of the gas is 27.3cm3 at 0oC. If the temperature is increased to 10oC while the pressure remains constant, we can use Charles's law to calculate the new volume of the gas. Charles's law states that the ratio of the initial volume to the initial temperature is equal to the ratio of the final volume to the final temperature. In other words: (V1 / T1) = (V2 / T2) Where: V1 = initial volume T1 = initial temperature V2 = final volume (unknown) T2 = final temperature Substituting the given values, we have: (27.3 / 273) = (V2 / 283) Solving for V2, we get: V2 = (27.3 / 273) x 283 V2 ≈ 28.3cm3 Therefore, the volume of the gas at 10oC, pressure remaining constant, is approximately 28.3cm3. Hence, the correct option is (ii) 28.3cm3.
Question 33 Report
The components of universal indicator solution can best be separated by
Answer Details
Universal indicator solution is a mixture of different indicators that changes color over a range of pH values. The best method to separate the components of universal indicator solution is chromatography. Chromatography is a method used to separate different components of a mixture based on their physical and chemical properties. In this case, the components of universal indicator solution can be separated based on their different solubility and adsorption properties. A small amount of the solution is placed on a chromatography paper and allowed to separate through the paper by capillary action. The different components of the mixture will travel at different rates based on their solubility in the solvent and their interaction with the paper. As a result, the different components can be separated and identified by their distinct color changes as they travel through the paper. Filtration, evaporation, crystallization, and fractional distillation are all separation methods that are based on the physical properties of the components of a mixture, such as their boiling points or solubility in a particular solvent. These methods are not suitable for separating the components of universal indicator solution, which are all indicators with similar physical properties.
Question 34 Report
Glucose can be obtained from starch by
Answer Details
Glucose can be obtained from starch by hydrolysis. Hydrolysis is a chemical reaction in which water is used to break down a compound into smaller molecules. In the case of starch, hydrolysis breaks down the long chains of glucose molecules into individual glucose molecules. This reaction is often catalyzed by enzymes such as amylase, which are found in saliva and the pancreas. The resulting glucose molecules can then be used by the body as a source of energy.
Question 35 Report
Calcium is usually extracted by the electrolysis of its
Answer Details
Calcium is usually extracted by the electrolysis of its chloride. Electrolysis is a process that involves the use of electrical energy to break down a compound into its constituent elements. In the case of calcium, the most common compound that it is extracted from is calcium chloride (CaCl2). Calcium chloride is an ionic compound, which means that it consists of positively charged calcium ions and negatively charged chloride ions. During electrolysis, an electric current is passed through a molten or dissolved compound, causing the ions to move towards the electrodes. At the negative electrode (cathode), the positively charged calcium ions gain electrons and are reduced to form calcium atoms. At the positive electrode (anode), the negatively charged chloride ions lose electrons and are oxidized to form chlorine gas. The overall reaction during the electrolysis of calcium chloride is: CaCl2(l) → Ca(l) + Cl2(g) This process is used to extract calcium on an industrial scale, as it is an efficient method for producing large quantities of calcium.
Question 36 Report
Destructive distillation of coal means
Answer Details
Destructive distillation of coal means heating coal in the absence of air. This process breaks down the complex organic compounds in coal into simpler molecules such as gases, liquids, and solids. These products are then collected and can be used for a variety of purposes such as the production of coal gas, tar, and coke. This process is called destructive distillation because the coal is being broken down or "destroyed" into simpler substances through the process of heating.
Question 37 Report
(a) Define oxidation in terms of electron transfer.
(b) Consider the following: Cu\(_{(s)}\) + 2Ag\(^{+}_{(Ag)}\) \(\to\) Cu\(^{2+}_{(aq)}\) + 2Ag\(_{(s)}\)
(i) State the species that is reduced
(ii) Write half-cell equation for each of the species.
Answer Details
None
Question 38 Report
(a) When MgSO\(_4\).XH\(_2\)O crystals were exposed to the atmosphere for several days, three was a loss in mass
(i) What name is given to this phenomenon?
(ii) Give another example of a compound that exhibits this phenomenon
(b) If 0.50 mole of MgSO\(_4\).XH\(_2\)O has a mass of 123g. calculate the value of X. (H = 1, O = 16, Mg = 24, S = 32)
Answer Details
None
Question 39 Report
(1)(a) State Avogadro's law
(b) Which of the state of matter contains particles that are: (i) readily used
(ii) held firmly together by some forces of cohesion;
(iii) involved in rapid random motion?
Question 40 Report
(a) Write an equation to show the action of strong heat on:
(i) potassium trioxonitrate (V):
(ii) sucrose.
(b) State two observations in respect of the reaction between granulated zinc and dilute tetraoxosulphate (VI) acid.
Question 41 Report
(a) Give one example each of a naturally occurring substance that;
(i) conforms to the general formula C(_x\)(H\(_2\)O)\(_y\);
(ii) contains the carboxyl group as its functional group.
(b) Name the process for obtaining: (i) paraffin oil from crude oil; (ii) benzene from ethyne.
Answer Details
None
Question 42 Report
(a)(i) What is meant by hydrocarbons?
(ii) A hydrocarbon consists of 92.3% carbon. If it's vapour density is 39, determine its molecular formula. (H = 1; C = 12)
(b)(i) Outline a suitable laboratory procedure for obtaining ethanol from cassava tubers
(ii) List two laboratory reagents used for oxidizing ethanol to ethanoic acid.
(c) What name is given to each of the following processes?:
(i) Conversion of alkanols to alkanoates;
(ii) Breakdown of proteins to amino acids;
(iii) Conversion of oils to fats
(iv) Alkaline hydrolysis of fats and oils.
None
Answer Details
None
Question 43 Report
Potassium trioxochlorate (V) undergoes thermal decomposition according to the fotpowing equation: 2KCIO\(_3\) \(\to\) 2KCI + 3O\(_2\)
(a) What substance could be used in the laboratory to in ease the rate of the reaction
(ii) absorb the oxygen produced
(b) Give the reason why an aqueous solution of silver trioxonitrate (V) gives a white precipitate with KCI but not with KClO\(_3\).
Answer Details
None
Question 44 Report
(a) State whether entropy increases or decreases during each of the following processes
(i) condensation of steam;
(ii) melting of wax;
(iii) dissolution of sugar in water;
(iv) abscas on charcoal.
(b) What deduction can be made in each case given that the value of the free energy change for a particular reaction is:
(i) zero;
ii) negative
Answer Details
None
Question 45 Report
A shortened form of the Periodic Table is shown below. Use it to answer questions (a) and (b)
(a) Which of the elements represented as A to E in the table, above is:
(i) transition metal;
(ii) an alkaline earth meta
(iii) the least reactive;
(iv) the most electronegative?
(b)(i) What type of bond would exist in a compound formed when element D reacts with oxygen?
(ii) Write the formula of the compound formed in (b)(i) above.
Answer Details
None
Question 46 Report
(a)(i) Draw a labelled diagram for the laboratory preparation of a dry sample of chlorine
(ii) Give one chemical test for chlorine.
(b) Write equations to represent the reaction of chlorine gas with: (i) iron (II) chloride solution;
(ii) potassium iodide solution;
(iii) hot concentrated sodium hydroxide solution.
(c) State what is observed on:
(i) bubbling hydrogen chloride gas into an solution of lead (II) trioxonitrate (V);
(ii) heating the mixture from (c)(i) above to boiling and aging it to cool.
(d) A solution of bismuth chloride was prepared by adding the oxychloride which is a white powder to concentrated hydrochloric acid. The following equilibrium was set up: BiOCI\(_{(s)}\) + 2HCI\(_{(aq)}\) \(\rightleftharpoons\) BiCl\(_{3(aq)}\) + H\(_2\)O\(_{(q)}\). State what would be observed if some water is added to the system. Explain your answer
Question 47 Report
(a) State two differences in the chemical properties of metals and non-metals.
(b) List two general methods of extract metals from their ores.
Answer Details
None
Question 48 Report
When ethane - 1,2-dioic acid is heated with concentrated tetraoxosulphate (VI) acid, a reaction represented by the following equation occurs:
(a) State the type of process involved in the reaction
(b) What is the basicity of ethane-1, s-dioic acid?
(c) List three differences in the chemical properties of the two oxides of carbon produced during the reaction
None
Answer Details
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Question 49 Report
(a)(i) Determine the maximum number of electrons that can occupy the principal energy level M of an atom.
(ii) Show the changes in the electronic structures of atoms of sodium and fluorine (\(^{23}_{11}\)Na: \(^{19}_{9}F\)) when they combine to form sodium fluoride.
(iii) State: three properties that sodium fluoride would have, based a-n the bond type present in the compound.
(b) Write equations to show when:
(i) sodium metal burns in limited supply of oxygen;
(ii) water is added to the product in (b)(i) above
(c) Describe a suitable laboratory procedure for comparing the conductance of 1 mol dm\(^{-3}\) aqueous solutions of sodium hydroxide and ethanoic acid.
None
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Question 50 Report
(a) (i) Define heat of combustion.
(ii) What name is given to the container used for determining tne reaction?
(b) The heat of combustion of carbon in excess air is - 3935 kJ.
(i) Sketch an energy profile diagram for the reaction.
(ii) Calculate the heat change when 60 g of carbon undergoes complete combustion to produce carbon (IV) oxide. (C = 12)
(iii) Explain why the value of the heat of neutralization of strong acids by strong bases is constant.
(c) Give reason for the following:
(i) rusting of iron is regarded as a slow combustion process;
(ii) iron filings rust much more faster than iron nails when exposed to the same atmospheric condition;
(iii) iron is better protected from corrosion by plating it with.zinc than with tin
Answer Details
None
