WAEC SSCE - Chemistry - 1990
Question 1 Report
To what temperature must a gas be raised from 273K in order to double both its volume and pressure?``
Answer Details
To double the pressure and volume of a gas, we need to use the combined gas law, which states that: (P1 × V1) / T1 = (P2 × V2) / T2 where P is the pressure, V is the volume, and T is the temperature of the gas. Let's assume that the initial temperature, pressure, and volume of the gas are T1 = 273 K, P1 = 1 atm, and V1 = 1 L, respectively. If we want to double both the pressure and volume of the gas, then the final values will be P2 = 2 atm and V2 = 2 L. Substituting these values into the combined gas law, we get: (1 atm × 1 L) / 273 K = (2 atm × 2 L) / T2 Solving for T2, we get: T2 = (2 atm × 2 L × 273 K) / (1 atm × 1 L) = 1092 K Therefore, the gas must be raised to a temperature of 1092 K in order to double both its volume and pressure.
Question 4 Report
Which of the following explains why trioxonitrate (V) acid is not used for preparing hydrogen from metals?
Answer Details
Trioxonitrate (V) acid (HNO3) is a strong oxidizing agent that can react with many metals, including those that can react with acids to form hydrogen gas. However, it does not produce hydrogen gas because it oxidizes the metal instead of producing hydrogen gas. The nitrate ion in the HNO3 oxidizes the metal to form an oxide layer on the surface of the metal, rendering it passive. This oxide layer prevents further reaction between the metal and the acid, and as a result, hydrogen gas is not produced. Therefore, trioxonitrate (V) acid is not used for preparing hydrogen from metals.
Question 5 Report
In the reaction represented by the equation; 2FeCI3 + SO2 + 2H2O → 2FeCL2 + H2SO4 + 2HCI the oxidation number of sulphur changes from
Answer Details
In the given chemical reaction, the oxidation number of sulfur changes from 4 in SO2 to 6 in H2SO4. Oxidation number is the charge an atom would have if the shared electrons were assigned to the more electronegative atom in a compound. In SO2, oxygen has an oxidation number of -2, and since there are two oxygen atoms, the total charge from oxygen is -4. Therefore, to balance the charge of SO2, sulfur has an oxidation number of +4. In H2SO4, oxygen still has an oxidation number of -2, and since there are four oxygen atoms, the total charge from oxygen is -8. Hydrogen has an oxidation number of +1, and there are two hydrogen atoms, for a total charge of +2. To balance the charge of H2SO4, sulfur must have an oxidation number of +6. Therefore, the oxidation number of sulfur changes from +4 to +6 in this reaction.
Question 6 Report
Which of the following equations represents the reaction leading to the removal of permanent hardness of water?
Question 7 Report
The heat accompanying the reaction represented by the equation H2O (l) → H 2O(g) is described as the heat of
Answer Details
The heat accompanying the reaction represented by the equation H2O(l) → H2O(g) is described as the heat of vaporization. This is because the process involves a change in the state of matter from liquid to gas, which requires energy to overcome the intermolecular forces of attraction between the water molecules. The energy required to vaporize a given amount of a substance is called the heat of vaporization. In this case, it is the amount of heat energy required to vaporize one mole of water at a constant temperature and pressure.
Question 9 Report
Which of the following is not correct of glucose and fructose?They
Question 10 Report
How many mole of AgNO 3 are there in 500cm3 of 0.01MAgNO3 solution?
Answer Details
To determine the number of moles of AgNO3 in a solution, we need to use the formula: moles = concentration x volume Here, the concentration is given as 0.01 M (M represents molarity, which is the number of moles of a solute per liter of solution), and the volume is given as 500 cm3 (cubic centimeters). However, we need to convert the volume to liters before we can use the formula. There are 1000 cm3 in 1 liter, so: 500 cm3 = 500/1000 L = 0.5 L Now we can use the formula: moles = 0.01 M x 0.5 L = 0.005 moles Therefore, the answer is 0.005 moles of AgNO3.
Question 11 Report
Which of the following compounds crystallizes without water of crystallization?
Answer Details
The compound that crystallizes without water of crystallization is NaCI (sodium chloride). When some compounds crystallize, they form a specific number of water molecules as part of their crystal structure. These water molecules are called water of crystallization. For example, CuSO4⋅5H2O means that each CuSO4 unit is bonded to 5 water molecules. However, NaCI does not form water of crystallization when it crystallizes. Instead, the sodium ions (Na+) and chloride ions (CI-) bond together in a lattice structure without any water molecules. This is why NaCI is known as an anhydrous compound. Therefore, the compound that crystallizes without water of crystallization is NaCI.
Question 12 Report
Which of the following salts in aqueous solution will have a pH greater than 7?
Answer Details
The salt that will have a pH greater than 7 in aqueous solution is K2CO3. When a salt is dissolved in water, it may undergo hydrolysis, which is a chemical reaction between the ions of the salt and the water molecules. Depending on the nature of the ions, the hydrolysis of a salt can result in an acidic, basic or neutral solution. K2CO3 is a salt of a strong base (KOH) and a weak acid (H2CO3). When it is dissolved in water, the carbonate ions react with water molecules to produce hydroxide ions (OH-) and bicarbonate ions (HCO3-). HCO3- + H2O ⇌ H3O+ + OH- The presence of hydroxide ions in solution makes it basic. Therefore, the pH of a solution of K2CO3 in water will be greater than 7. In contrast, NaCl, ACI3, FeCI3, and Na2SO4 do not contain hydroxide ions or any other ions that can significantly affect the pH of the solution. They will therefore result in neutral solutions with a pH of 7. Therefore, the answer is K2CO3, because it is the only salt of the options given that will produce a basic solution with a pH greater than 7.
Question 13 Report
The gas that is liberated when iron is heated with concentrated tetraoxosulphate (VI)acid is
Question 14 Report
The following alloys contain copper except
Answer Details
The alloy that does not contain copper is magnalium. Bronze and brass are copper alloys. Bronze is an alloy of copper and tin, while brass is an alloy of copper and zinc. Duralumin is an alloy of aluminum, copper, and magnesium. Type metal is an alloy of lead, tin, and antimony. Magnalium is an aluminum alloy that contains magnesium but not copper. Therefore, the answer is magnalium as it is the only option that does not contain copper.
Question 15 Report
Which of the following statements explains why tetraoxosulphate (IV) acid is reqarded as a strong acid?
Answer Details
The statement that explains why tetraoxosulphate (IV) acid is regarded as a strong acid is that the acid is completely ionized in aqueous solution. This means that when tetraoxosulphate (IV) acid dissolves in water, all the acid molecules dissociate into ions. In the case of tetraoxosulphate (IV) acid, the hydrogen ion (H+) and tetraoxosulphate (IV) ion (SO4²-) are formed when it dissolves in water. The completeness of ionization of a strong acid in aqueous solution is due to the stability of the resulting ions, which are highly charged and polar. This means that the ions are strongly attracted to the water molecules, making it difficult for them to recombine and reform the original acid molecule. As a result, the concentration of H+ ions in the solution is high, leading to a low pH value. In contrast, weak acids are only partially ionized in aqueous solution, meaning that only a fraction of the acid molecules dissociate into ions. This is due to the fact that the resulting ions are not as stable as those produced by strong acids. As a result, the concentration of H+ ions in a weak acid solution is lower, leading to a higher pH value. Therefore, tetraoxosulphate (IV) acid is regarded as a strong acid because it completely ionizes in aqueous solution, leading to a high concentration of H+ ions and a low pH value.
Question 16 Report
MO and X 2O represent the formula of oxides of elements M and X respectively . If M and X should combine to form a separate compound, what would be the formula of the compound?
Answer Details
Question 17 Report
The compound of copper which is used in electroplating dyeing, printing, wood preservation and as a fungicide is
Answer Details
The compound of copper which is used in electroplating dyeing, printing, wood preservation and as a fungicide is copper (ll) tetraoxosulphate (VI) pentahydrate, also known as copper sulphate. Copper sulphate is a blue crystalline solid that contains copper, sulphur, and oxygen. It is commonly used in electroplating to coat objects with a thin layer of copper. It is also used as a mordant in dyeing and printing fabrics, to preserve wood, and as a fungicide in agriculture. Other compounds of copper listed in the options, such as copper (ll) hydroxide, copper (ll) trioxonitrate (V) pentahydrate, copper (ll) oxide, and copper (ll) trioxocarbonate (lV) are also used for various purposes. However, copper sulphate is the specific compound used in the applications mentioned in the question.
Question 18 Report
A sample of orange juice is suspected to have been contaminated with a yellow dye. Which of the following methods can be used to detect the dye?
Answer Details
Chromatography can be used to detect the yellow dye in the sample of orange juice suspected to be contaminated. Chromatography is a technique used to separate mixtures of substances into their individual components. It works by passing a mixture through a stationary phase, which is typically a solid or a liquid supported on a solid, and a mobile phase, which is typically a liquid or a gas. The components in the mixture separate out based on their interactions with the stationary and mobile phases, and can be identified by their distinct positions on the stationary phase. In this case, the orange juice sample suspected to be contaminated with the yellow dye can be passed through a chromatographic column, and the dye can be separated from the other components in the sample based on its interactions with the stationary and mobile phases. Once the dye is separated, it can be identified by its characteristic position on the stationary phase or by using other analytical techniques. Therefore, the correct answer is "Chromatography".
Question 19 Report
Which of the following compounds will undergo additional reactions?
Answer Details
Ethyne (also known as acetylene) is the compound that will undergo additional reactions. Ethyne has a triple bond between the two carbon atoms, which is a reactive functional group that can easily participate in addition reactions with other compounds. Additionally, the sp hybridization of the carbon atoms in the triple bond makes them more electronegative and reactive towards electrophiles. In contrast, butane, pentane, and tetrachloromethane are saturated hydrocarbons that do not have any reactive functional groups and are not expected to undergo additional reactions. Ethanol has an -OH functional group, but it is also saturated and does not undergo additional reactions under normal conditions.
Question 20 Report
Which of the following pollutants is biodegradable ?
Answer Details
Sewage is a pollutant that is biodegradable. Biodegradable means that the substance can be broken down naturally by microorganisms into simpler substances, such as water and carbon dioxide. Sewage contains organic matter that can be easily decomposed by bacteria, which is why it is considered biodegradable. This is also why wastewater treatment plants use bacteria to break down organic matter in sewage before releasing it into the environment. Plastics, metal scrap, lead compounds, and hydrogen sulfide are not biodegradable pollutants. Plastics can take hundreds of years to decompose, and even then, they only break down into smaller plastic particles that can cause harm to the environment and wildlife. Metal scrap and lead compounds do not break down naturally and can accumulate in the environment over time, leading to toxicity issues. Hydrogen sulfide is a gas that can be toxic to living organisms, but it does not biodegrade as it is a simple molecule that does not contain carbon.
Question 22 Report
Which of the following reactions does not occur in the blast furnace during the extraction of iron?
Answer Details
Question 23 Report
Which of the following reaction will not take place under normal conditions?
Answer Details
Question 24 Report
Catalytic hydrogenation of oils results in the production of
Answer Details
The catalytic hydrogenation of oils involves adding hydrogen gas to unsaturated fats, which are commonly found in vegetable oils, to create a more saturated fat. This process is commonly used to produce margarine and other types of spreads. During this process, the double bonds in the unsaturated fats are broken, and hydrogen atoms are added to the carbon atoms to create single bonds. This results in the formation of more saturated fats, which are typically solid at room temperature and have a longer shelf life. Therefore, the catalytic hydrogenation of oils results in the production of more saturated fats, which can be used to create products such as margarine, rather than soaps, detergents or alkanes. Butter is a natural product made from milk fat and is not typically produced through catalytic hydrogenation.
Question 25 Report
How many molecules are there in 14g of nitrogen gas at s.t.p? (n = 14, Avogadro Number = 6. 0 x 1023 mol-1)
Question 26 Report
Which of the following correctly explains entropy?
Question 27 Report
What is the molecular formula of a compound whose empirical formula is CH2O and molar mass is 180? (H = 1, C = 12, O = 16)
Answer Details
The empirical formula of a compound gives the simplest whole number ratio of the atoms present in it. To determine the molecular formula of a compound from its empirical formula and molar mass, we need to find the actual number of atoms of each element in the molecule. In this case, the empirical formula of the compound is CH2O, which has a molar mass of 30 (12 for carbon, 2 for hydrogen, and 16 for oxygen). However, the molar mass of the compound is given as 180 g/mol, which is six times larger than the empirical formula. To find the molecular formula, we need to multiply the empirical formula by a whole number n that gives the actual number of atoms of each element in the molecule. Since the molar mass of the compound is six times larger than its empirical formula, we can assume that the molecular formula is six times larger than the empirical formula. Therefore, we can write: Empirical formula mass = 30 g/mol Molecular formula mass = 6 x empirical formula mass = 6 x 30 g/mol = 180 g/mol The molecular formula will have 6 times the number of atoms as the empirical formula. Thus, the molecular formula of the compound is C6H12O6
Question 29 Report
The decomposition of hydrogen peroxide is represented by the equation: 2H2O(l) + O2(g) what mass of hydrogen peroxide would be required to produce 22.4dm3 of oxygen at s.t.p? (H = 1, O = 16, molar volume of a gas at s.t.p. = 22.4dm3)
Answer Details
The balanced chemical equation for the decomposition of hydrogen peroxide is: 2H2O2(l) → 2H2O(l) + O2(g) From the equation, it is clear that 2 moles of hydrogen peroxide will produce 1 mole of oxygen gas. Also, 1 mole of any gas at s.t.p. occupies a volume of 22.4 dm3. Therefore, to produce 22.4 dm3 of oxygen gas, we need 2 moles of hydrogen peroxide. This is because 2 moles of hydrogen peroxide will produce 1 mole of oxygen gas. Now, we can use the molar mass of hydrogen peroxide to find the mass of hydrogen peroxide needed. The molar mass of hydrogen peroxide (H2O2) is: 2(1.01) + 2(16.00) = 34.02 g/mol So, 2 moles of hydrogen peroxide will have a mass of: 2 mol x 34.02 g/mol = 68.04 g Therefore, 68.04 g of hydrogen peroxide is required to produce 22.4 dm3 of oxygen gas at s.t.p. Thus, the answer is (E) 68 g.
Question 30 Report
A catayst which increases the rate of a chemical reaction does so by
Answer Details
A catalyst increases the rate of a chemical reaction by decreasing the activation energy required for the reaction to occur. In simpler terms, the catalyst provides an alternative pathway for the reaction to take place, which requires less energy than the original pathway. This lower energy pathway allows more reactant molecules to collide with enough energy to overcome the activation energy barrier, which speeds up the rate of the reaction. Therefore, a catalyst does not change the initial or final energy levels of the reaction, but it lowers the energy barrier that must be overcome for the reaction to take place, making the reaction occur more quickly.
Question 31 Report
Aluminum is above iron in the electrochemical series, yet iron corrodes easily on exposure to air while aluminium does not. This is because aluminium
Answer Details
Aluminum does not corrode easily on exposure to air while iron does, even though aluminum is above iron in the electrochemical series. This is because aluminum forms a thin layer of inert oxide (Al2O3) on its surface when exposed to moist air, which acts as a protective layer and prevents further corrosion. On the other hand, iron does not form a stable oxide layer and hence corrodes easily. Therefore, the correct answer is "forms a thin layer of inert oxide in moist air".
Question 32 Report
The following metals are extracted by the electrolytic method except
Answer Details
Question 33 Report
(a) Give the formula indicating the relationship between entropy, free energy and enthalpy changes of a system.
(b) For each of the following, state whether entropy change is positive, negative or zero.
(i) H\(_2\)O\(_{(g)}\) -> H\(_2\)O\(_{(g)}\)
(ii) Cl\(_{2(g)}\) ---> 2CI\(_{(g)}\)
(iii) HCI\(_{(g)}\) -> HCl\(_{(g)}\)
Question 34 Report
(a) Balance the nuclear equation below and hence identify Y.
\(^{238}_{234}U \to ^{234}_{92}Th + Y\)
(b) In.a tabular form, state two of the observations in the cathode ray experiment and the corresponding deductions.
Answer Details
None
Question 35 Report
(a) Write the electronic configuration of an element with atomic number 15, indicating the distribution of electrons in the energy sub-levels
(b) Give the formula and the colour of the complex formed between ammonia and copper (II) ions
Question 36 Report
A hydrocarbon X which decolorizes bromine water but has no action on ammoniacal silver trioxonitrate (V) solution was found to have a molar mass of 58 g mol\(^{-1}\)
(a) Deduce the molecular formula of X. (H = 1, C = 12)
(b) Write the structures of two isomers of X.
Question 37 Report
(a)(i) Define the term addition polymerization
(ii) What type of organic compounds undergo addition polymerization
(iii) List two factors which affect the strength of polymers
(b) The diagram below shows some reaction pathways involving ethanol
(i) Write the name and structural of the organic product X
(ii) State the reagent for the conversation indicated as step A.
(iii) What type of reaction will ethanol undergo CH\(_3\)CH\(_2\)COOH during the process of conversation indicated as step B?
(c)(i) Write three balanced equation for the complete combustion of ethanol in :date the volume of oxygen required at s.t.p for the complete combustion of ethanol. (H = 1, C = 12, O = 16, molar volume of gases at s.t.p. = 22.4 dm\(^3\))
(d)( i} State two substances produced when coal is heated in the absence of air
(ii) What name is given to the process in (d)(i) above?
(iii) State the importance of the non-volatile residue of the process named in (d)(iii) to the iron and steel industry.
Question 38 Report
Benzene contains six carbon atoms and six hydrogen atoms.
(a)(i) Draw two stable structures of benzene to show how these atoms are arranged.
(ii) What is the concept behind these structures?
(b) Give (i) two uses of benzene. (ii) one industrial source of benzene.
Question 39 Report
(a) Arrange the first three members of the halogen family in their increasing order of electronegativity. Give the reason for your answer.
(b) State and explain what happens when chlorine reacts with starch iodide paper.
Question 40 Report
(a) Give one reason why a collision between reactants may not produce new species.
(b) Explain, illustrating with appropriate equation(s), why an aqueous solution of aluminium chloride is acidic.
Answer Details
None
Question 41 Report
(a) Name the type of solid structure possessed by:
(i) diamond;
(ii) iodine;
(iii) sodium chloride.
(b) Give:
(i) one alloy of tin:
(ii) a common reducing agent which is a compound of tin.
Answer Details
None
Question 42 Report
Liquefied air is mainly a mixture of nitrogen and oxygen which can be separated into its components by fractional distillation (Boiling point of nitrogen is 196°C, Boiling point of oxygen is 174°C)
(a) Name the fraction which distills over first. Give the reason for your answer.
(b) Give another industrial application of fractional distillation as a separation technique.
Answer Details
None
Question 43 Report
Consider the reaction represented by the equation: 2SO\(_{2(g)}\) + O\(_{2(g)}\) 
2SO\(_{3(g)}\). \(\Delta\)H = 188KJ.
(a) Write an expression for the equilibrium constant
(b) Sketch an energy diagram for the forward reaction, showing the profile for the catalyzed and non-catalyzed systems.
(c) state the reason, the effect of the following on the position of equilibrium of the system:
(i) increase in temperature
(ii) increase in pressure;
(iii) removal of some of the SO\(_3\) produced;
(iv) presence of V\(_2\)O\(_5\)
(d)(i) Write equations to show how the sulphur(VI) oxide is converted to tetraoxosulphate(VI) acid in the contact process
(ii) Give two uses of tetraoxosulphate(VI) acid.
Answer Details
None
Question 44 Report
(a) Give two reasons why carbon(IV) oxide is used for extinguishing fire
(b) Explain briefly the water softening action of cation exchane resins.
Answer Details
None
Question 45 Report
(a)(i) List two physical properties used as criteria for purity of substances
(ii) describe how you would prepare a pure, dry sample of sodium chloride crystals by a neutralization reaction, using bench reagents.
(iii) Give two other general methods for preparing soluble salts.
(b) Explain the following observations:
(i) a sheet of iron placed in dilute copper (II) tetraoxosulphate (VI) solution reddish brown;
(ii) the white gelatinous precipitate formed when a few drops of sodium hydroxide solution are added to a solution of aluminium salt dissolves in excess alkali;
(iii) the pale green prepared iron(II) chloride solution changes to brown on bubbling chlorine gas through it.
(iv) Write a balanced equation for the reaction of dilute hydrochloric acid with marble. List two industrial process in which limestone is used as a raw material.
Answer Details
None
Question 46 Report
(a)(i) Define oxidation in terms of electron transfer.
(ii) Write balanced equations for the half reactions for the following changes in acidic solution: Mn0\(^-_4\) + Fe\(^{2+}\) —> Mn\(^{2+}\) + Fe\(^{3+}\)
(b)(i) Distinguish between an electrolytic celI and an electrochemical cell.
(ii) Sketch a cell for the electrolysis of molten magnesium chloride. Lable the anode and the cathode and indicate the direction of electron flow. Give the electrode reactions.
(iii) Give one reason why a platinum anode is not suitable for the eloctrolysis in (b)(i) above.
(c) Calculate the mass of lead that would be deposited from a solution of lead (II) trioxonitrate by the same quantity of electrically depositing 1.35g of copper. (Cu = 63.5, Pb = 207)
Answer Details
None
