WAEC SSCE - Chemistry - 1989
Question 1 Report
Which of the following is a condition for a spontaneous reaction?
Answer Details
The condition for a spontaneous reaction is that the Gibbs free energy change (∆G) of the system should be negative. ∆G is related to enthalpy change (∆H), entropy change (∆S), and temperature (T) through the equation: ∆G = ∆H - T∆S For a spontaneous reaction, ∆G must be negative, which can only occur when one of the following conditions is met: - ∆H is negative (exothermic reaction) and ∆S is positive (increase in disorder) - ∆H is positive (endothermic reaction) and ∆S is negative (decrease in disorder), but T∆S is larger than ∆H, so the overall ∆G is negative. Therefore, the option that represents a condition for a spontaneous reaction is: ∆H-T∆S is negative.
Question 2 Report
Given that for the reaction. N2(g) + 3H2(g) ⇌ 2NH3(g) ∆H = -92kJ. What is the enthalpy of formation of ammonia from its elements?
Question 3 Report
The oxidation number of chlorine is + 1 in
Answer Details
The oxidation number of an atom is the charge it would have if electrons were transferred completely to the more electronegative atom. Chlorine is more electronegative than most other elements, and thus has a high tendency to gain electrons. The oxidation number of chlorine in KCIO3 is +5, in CI2O7 is +7, in ZnCI2 is -1, and in HCI is -1. Therefore, the only option where the oxidation number of chlorine is +1 is NaCIO.
Question 4 Report
The rate of the hydrogen in the reaction Zn(s) + 2HCI (aq) → ZnCI 2(g) + H 2(aq) + H 2(g) can be increased by
Answer Details
Question 5 Report
When an element can exist in two or more forms in the same physical state, the element is said to exhibit
Answer Details
The correct answer is allotropy. Allotropy is a phenomenon in which an element can exist in two or more different physical forms, known as allotropes, in the same physical state (i.e., solid, liquid, or gas) under different conditions of temperature and pressure. The different allotropes of an element have different physical and chemical properties, such as density, melting point, and reactivity, due to differences in their molecular or crystal structures. Some examples of elements that exhibit allotropy include carbon (which has the allotropes graphite, diamond, and fullerenes), oxygen (which has the allotropes O2 and O3), and sulfur (which has the allotropes S8, S6, and S4).
Question 6 Report
Copper can best be purified by
Answer Details
Copper can best be purified by electrolyzing a copper (ll) salt solution using the impure copper as the anode. Electrolysis is a process in which an electric current is passed through a solution containing ions, causing them to move towards the electrodes. In this case, the impure copper is used as the anode, and the cathode is made of pure copper. As the current passes through the solution, the impure copper anode dissolves, and the copper ions move towards the cathode and are deposited as pure copper. This process allows for the removal of impurities from the copper, resulting in a higher level of purity than other methods such as roasting or heating with coke.
Question 7 Report
Which of the following carbohydrates does NOT usually occur in the crystalline form?
Answer Details
Cellulose does not usually occur in the crystalline form. Cellulose is a complex carbohydrate that forms long, linear chains of glucose molecules, which are linked by beta-glycosidic bonds. The chains form bundles, which are stabilized by hydrogen bonds. These bundles further form microfibrils, which make up the structural material of plants. Although cellulose has a regular and repeating structure, it does not form crystals because of its complex and branched structure. In contrast, glucose and sucrose can form crystals, and maltose and fructose can occur in both crystalline and amorphous forms.
Question 8 Report
What quantity of copper will be deposited by the same quantity of electricity that deposited 9.0g of aluminum? (A = 27, Cu = 64)
Answer Details
Question 9 Report
Which of the following is used extensively in manufacturing photographic chemicals?
Answer Details
Silver chloride is used extensively in manufacturing photographic chemicals. It is a light-sensitive compound that is used in making photographic paper and film. When exposed to light, it undergoes a chemical reaction that results in the formation of a visible image. Silver chloride is also used in making emulsions and toners for black and white photography.
Question 10 Report
50cm 3 of a saturated solution of potassium trioxonitrate (V)at 40°C contains 5.05g of the salt. What is the solubility of potassium trioxonitrate (V) at 40°C? (KNO3 = 101)
Answer Details
The solubility of a substance is the maximum amount of solute that can be dissolved in a given amount of solvent at a specific temperature. In this question, we are given the volume and concentration of a saturated solution of potassium trioxonitrate (V) at 40°C. We can use this information to calculate the solubility of the salt at 40°C. First, we need to convert the given volume from cm3 to dm3 (litres) since the concentration is given in mol dm-3. 50 cm3 = 50 ÷ 1000 dm3 = 0.05 dm3 The number of moles of potassium trioxonitrate (V) in the solution can be calculated using the formula: moles = concentration × volume The concentration is given as saturated, which means that the solution contains the maximum amount of potassium trioxonitrate (V) that can dissolve at 40°C. Therefore, the concentration is equal to the solubility of the salt at that temperature. So, we have: moles of KNO3 = solubility × volume = solubility × 0.05 dm3 We are also given the mass of KNO3 in the solution, which is 5.05 g. We can use the molar mass of KNO3 (101 g/mol) to calculate the number of moles: moles of KNO3 = mass ÷ molar mass = 5.05 ÷ 101 = 0.05 mol Now, we can equate the two expressions for the number of moles of KNO3: solubility × 0.05 = 0.05 solubility = 0.05 ÷ 0.05 = 1 mol dm-3 Therefore, the solubility of potassium trioxonitrate (V) at 40°C is 1.0 mol dm-3. Answer: 1.0 mol dm-3.
Question 11 Report
If 200cm 3 of a gas at s.t.p. has a mass of 0.268g, what is its molar mass? (Molar volume of a gas at s.t.p. = 22.4 dm3)
Answer Details
The molar mass of a gas can be calculated using the following formula: molar mass = mass ÷ number of moles At standard temperature and pressure (STP), the molar volume of a gas is 22.4 dm3, which is equivalent to 22,400 cm3. Therefore, the number of moles of the gas can be calculated as follows: number of moles = volume of gas at STP ÷ molar volume of gas at STP number of moles = 200 cm3 ÷ 22,400 cm3/mol number of moles = 0.00893 mol Now, we can use the formula for molar mass to find the answer: molar mass = mass ÷ number of moles molar mass = 0.268 g ÷ 0.00893 mol molar mass = 30.03 g/mol Therefore, the molar mass of the gas is approximately 30 g/mol. The correct answer is.
Question 12 Report
Given that for the reaction KOH (aq) + HCI(aq) → KCI(aq) + H2O(L) H = - 54 Kj mol-1. What is the quantity of heat involved in the reaction?2NaOH(aq) + H2SO 4(aq) → Na2SO4(aq) + 2H 2O(l)?
Answer Details
Question 13 Report
The following are miscible with water except
Answer Details
Among the given options, ethylethanoate, methanol, ethanoic acid, methanoic acid, and ethanol are all polar substances, meaning they have a partially positive and partially negative end due to the arrangement of their atoms. These partial charges allow them to interact with water molecules through hydrogen bonding, making them soluble or miscible in water. However, ethylethanoate is the only exception since it is a nonpolar substance. It lacks partial charges, and as such, cannot form hydrogen bonds with water molecules, making it insoluble or immiscible in water.
Question 14 Report
If sulphur is dissolved in carbon (IV) sulphide and the solution is allowed to evaporate, the allotrope of sulphur formed is
Answer Details
Question 15 Report
Which of the following statements is not true of tin? it
Answer Details
The statement that is not true of tin is that it combines with copper to form the alloy brass. Brass is actually an alloy of copper and zinc, not copper and tin. All the other statements are true of tin. Tin is a p-block element, it is extracted from cassiterite SnO2, it is used for protecting iron containers from corrosion, and it shows two oxidation states, +2 and +4 in most of its compounds.
Question 16 Report
What is the concentration, in mol dm 3, of solution is allowed to evaporate the allotrope of sulphur formed is
Answer Details
The formation of allotropes of sulphur is dependent on the concentration of the sulphur solution. If the concentration of the sulphur solution is high, then the allotrope of sulphur formed would be rhombic sulphur. However, if the concentration of the sulphur solution is low, then the allotrope of sulphur formed would be amorphous sulphur. Therefore, the concentration of the solution determines the allotrope of sulphur formed during evaporation.
Question 17 Report
Which of the following gases will bleach moist litmus paper?
Question 18 Report
The most suitable method to use when separating an insoluble solid from a liquid is
Answer Details
The most suitable method to use when separating an insoluble solid from a liquid is filtration. Filtration is a process of separating a solid from a liquid by passing the mixture through a porous material, such as filter paper or a sand bed. The solid is trapped on the filter paper, while the liquid passes through and is collected in a separate container. This method is effective for separating a solid that does not dissolve in the liquid, such as sand from water. Evaporation, magnetization, sublimation, and distillation are methods used for separating a solid from a liquid when the solid is either soluble in the liquid or has a different boiling point than the liquid.
Question 19 Report
Given the following half-cell reaction; 2Cl(aq) → CI2(g) + 2e, how many mole of electrons will be required to produce 1.12dm3 of chlorine gas at s.t.p? (Molar volume of a gas at s.t.p. = 22.4dm 3)
Question 20 Report
The electronic configuration of two atoms X and Y are as follows: X - 1s 2 2s 22p 63s 1, Y -1s 22s 22p 63s23p 64s 2 which of the statements below is true of the position of X and Y in the Periodic Table?
Answer Details
The electron configuration of X is 1s2 2s2 2p6 3s1 which indicates that X has one valence electron in its outermost shell. The valence electron of X is in the 3s subshell, which means that X is in period 3 of the periodic table. The electron configuration of Y is 1s2 2s2 2p6 3s2 3p6 4s2, indicating that Y has two valence electrons in its outermost shell. The valence electrons of Y are in the 4s subshell, which means that Y is in period 4 of the periodic table. Therefore, X belongs to group 1, and Y belongs to period 4, which means that the correct option is: "x belongs to group 1, Y belongs to period 4."
Question 21 Report
What is the voltage of the cell represented at Zn(s) Zn 2+(aq) /Cu2+(aq) /Cu(s) given that for Cu 2+(aq)/ Cu (s) Eo = 0.337V and for Zn2+(aq) /Zn(s)' E o = -0.763V?
Answer Details
The voltage of the cell can be calculated using the formula: Ecell = Ereduction, cathode - Eoxidation, anode The half-reactions for the cell are: Cathode: Cu2+ (aq) + 2e- → Cu(s) (Ereduction, cathode = 0.337V) Anode: Zn(s) → Zn2+ (aq) + 2e- (Eoxidation, anode = -0.763V) Substituting the values into the formula, we get: Ecell = 0.337V - (-0.763V) = 1.1V Therefore, the voltage of the cell represented at Zn(s) Zn 2+(aq) /Cu2+(aq) /Cu(s) is +1.10V. Answer: +1.10V
Question 22 Report
Given that 1 mole of carbon -12 weighs 12.0g, how many atoms are there in 24.0g magnesium? (C = 12, Mg = 24, NA = 6.02 x 10 23mol-1)
Answer Details
The molar mass of magnesium is 24.0 g/mol, which means that one mole of magnesium has a mass of 24.0 g. To find the number of atoms in 24.0 g of magnesium, we need to first determine the number of moles of magnesium in 24.0 g. We can do this using the formula: moles = mass/molar mass moles of magnesium = 24.0 g / 24.0 g/mol moles of magnesium = 1.0 mol So, there is 1.0 mole of magnesium in 24.0 g. We can use Avogadro's number (6.02 x 10^23) to find the number of atoms in 1.0 mole of magnesium: number of atoms = Avogadro's number x moles of magnesium number of atoms = 6.02 x 10^23 x 1.0 number of atoms = 6.02 x 10^23 Therefore, there are 6.02 x 10^23 atoms in 24.0 g of magnesium. The answer is 1 x 6.02 x 10^23.
Question 23 Report
The earthly impurities in iron ore are removed in the blast furnace by the reaction
Answer Details
Question 24 Report
120cm3 of hydrogen were sparked with 60cm 3 of oxygen at 110oC. What was the volume of stream produced? The equation for the reaction is 2H2(g) + O2(g) → 2H2O(g)
Question 25 Report
Why is potassium fluoride added to the electrolyte in the extraction of sodium from fused sodium chloride?
Answer Details
Question 26 Report
Which of the following hydrocarbons is not likely to be present in petrol?
Answer Details
Petrol is a complex mixture of hydrocarbons obtained from petroleum, and the composition of petrol can vary depending on its source and refining process. However, hydrocarbons with a higher number of carbon atoms tend to have higher boiling points and are more likely to be present in diesel or other heavier fuels rather than petrol. Therefore, the hydrocarbon that is not likely to be present in petrol is C14H30.
Question 27 Report
The following are s-block elements except
Answer Details
The s-block elements are the elements in Group 1 and Group 2 of the periodic table, plus hydrogen and helium. They are called "s-block" elements because their valence (outermost) electrons are in the s subshell of their atoms. Aluminium is not an s-block element. It is located in Group 13, which is part of the p-block elements. Its valence electrons are in the p subshell of its atoms. Therefore, the answer is aluminium.
Question 28 Report
The major raw material in a plastic industry is
Answer Details
The major raw material in a plastic industry is ethene. Ethene, also known as ethylene, is a colorless gas that is derived from natural gas or petroleum. It is the most commonly used monomer, or building block, in the production of plastic. Ethene is polymerized to form polyethylene, which is used in a wide variety of plastic products, including packaging materials, toys, and household items. The production of plastic from ethene is a highly energy-intensive process and contributes to the emission of greenhouse gases, which can have negative impacts on the environment and climate change.
Question 29 Report
How many carbon atoms are there in a benzene ring?
Answer Details
There are 6 carbon atoms in a benzene ring. Benzene is a colorless, highly flammable liquid that is composed of carbon and hydrogen atoms. Its molecular formula is C6H6, which means it contains six carbon atoms and six hydrogen atoms. The carbon atoms are arranged in a unique hexagonal ring structure, which is sometimes referred to as an aromatic ring. This ring structure gives benzene its distinctive chemical and physical properties and makes it an important building block for the production of many chemicals and materials, including plastics, rubber, and dyes.
Question 30 Report
Locally produced soap in which wood ash is used as the base is usually soft because the wood ash contains a lot of
Answer Details
Locally produced soap in which wood ash is used as the base is usually soft because the wood ash contains a lot of potassium ions. Potassium hydroxide, also known as caustic potash, is formed when wood ash is mixed with water. It is a strong alkali that reacts with fats and oils in the soap-making process to form soap molecules. Potassium ions are responsible for making the soap soft because they have a weaker attraction to water molecules than sodium ions, which are used in the production of hard soap. Therefore, soap made from potassium ions tends to be softer and more soluble in water.
Question 31 Report
Which of the following reactions represents the laboratory preparation of hydrogen?
Answer Details
The reaction that represents the laboratory preparation of hydrogen is Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g). In this reaction, zinc metal reacts with hydrochloric acid to produce hydrogen gas and zinc chloride. The other reactions do not produce hydrogen gas as one of their products or involve hydrogen gas as a reactant.
Question 32 Report
Which of the following statements best explains cracking ? It is a process
Answer Details
Cracking is a process in which large hydrocarbon molecules are broken down into smaller molecules. This is usually achieved by heating the hydrocarbon molecules to high temperatures and then passing them over a catalyst. Cracking is an important process in the petroleum industry because it allows for the production of smaller, more useful hydrocarbons, such as gasoline and diesel fuel, from larger, less useful ones, such as heavy oils and waxes. The smaller hydrocarbons produced by cracking have higher commercial value and are in greater demand for use as fuels, solvents, and raw materials for the production of other chemicals. Therefore, the answer is in which large hydrocarbon molecules are broken into smaller units.
Question 33 Report
Octane number is highest in petrol containing a high proportion of
Answer Details
Octane number is a measure of the performance of petrol in internal combustion engines. It is a rating based on the ability of petrol to resist 'knocking' or 'pinging' during combustion. Knocking or pinging is an undesirable condition that occurs when the air-fuel mixture in the engine's cylinder detonates prematurely, which can cause engine damage. A high octane number indicates that the petrol can resist knocking, allowing the engine to operate at higher compression ratios, which typically results in more power and efficiency. Therefore, petrol containing a high proportion of compounds with high resistance to knocking, such as 2,2,4-trimethylpentane (also known as iso-octane), will have a higher octane number. Hence, the correct option is 2,2,4-trimethylpentane.
Question 34 Report
(a) Distinguish between a conductor and an electrolyte
(b)(i) State Faraday's first law of electrolysis
(ii) Describe how you would investigate Faraday's law of electrolysis, using copper (II) tetraoxosulphate (VI) solution and copper electrodes.
(c) 0.222g of a divalent metal is deposited when a current of 0.45 ampere is passed through a solution of its salt for 25 minutes using appropriate electrodes. Calculate the relative atomic mass of the metal. 1F = 96500C mol\(^{-1}\)
`(d) State two applications of electrolysis.
Answer Details
None
Question 35 Report
Name the type of chemical process involved in the production of
(a) polythene from ethene
(b) ethene from kerosene fraction of petroleum.
(c) soap from vegetable oils
(d) margarine from vegetable oils
Answer Details
None
Question 36 Report
(a) Give one physical property of
(i) diamond;
(ii) graphite
(b) Give two uses of diamond
(c) evidence that shows that both graphite and diamond are allotropes of carbon.
Answer Details
None
Question 37 Report
(a) Write the formula of the oxide of nitrogen in which nitrogen has oxidation number of (i) +1;
(ii) +2;
(iii) +3;
(iv) +4;
(b) State which of the oxides in (a) above is/are: (i) acidic (ii) neutral.
Answer Details
None
Question 38 Report
Consider the compounds represented as A and B below:
(a) What is the celationship between A and B? (
b) Name A and B.
(c) Will the chemical properties of A and B be the same? Give one reason for your answer.
Answer Details
None
Question 39 Report
(a) Write the chemical equation for the formation of named alkanoate.
(b)(i) What are the monomers of protein called?
(ii) Write the two functional groups present in the monomers named in (b)(i) above
(iii) State the type of reaction that leads to the formation of proteins from their monomers.
Question 40 Report
(a) The half-life of 56/25 Mn is 9.3 x 10\(^3\)S. What does the statement mean?
(b) Give the three types of radiation that are usually emitted by radioactive substances.
Answer Details
None
Question 41 Report
(a) Name the components of
(i) producer gas; (ii) water gas;
(b) Give the reason why water is a better fuel than producer gas.
None
Answer Details
None
Question 42 Report
(a) Give two characteristic features of boiling
(b) What will be the effect of the following on the boiling point of water:
(i) addition of crystals of sodium chloride,
(ii) reduction of the atmospheric pressure?
(c) State two ways in which boiling differs from evaporation.
Answer Details
None
Question 43 Report
(a) List three characteristics of a homologous series
(b) Give one example of;
(i) alkanes; (ii) alkynes.
(c) A hydrocarbon contains 7.7% by mass of hydrogen and 92.3% by mass of carbon. The relative molar mass of the compound is 78.
(i) Derive the empirical formula of the compound and hence its molecular formula.
(ii) Name the hydrocarbon and write its structural formula. (H=1, C=12)
(d) Two hydrocarbons, X and Y were treated separated with acidified potassium tetraoxomanganate (VII) solution. X decolorized the solution and Y did not. Which of X and Y will undergo
(i) substitution reaction only,
(ii) both addition and substitution reactions.
(iii) polymerization?
(e) If ethanol is to be converted into ethanoic acid
(i) What are the conditions required?
(ii) name the type of reaction that will be involved and write the equation
Question 44 Report
(a) Explain the differences in the reactions of zinc with dilute trioxonitrate (V) acid and zinc with dilute hydrochloric acid.
(b) Write equations to illustrate how ammonia gas can be converted into trioxonitrate (V) acid.
(c) Calculate the mass of sodium trioxonitrate (V) produced when 30.0g of pure sodium hydroxide reacts with 100cm\(^3\) of 1.00 M trioxonitrate (V) acid. (H =1, N = 14, 0 = 16, Na = 23)
(d) Write the equations for the decomposition by heat of:
(i) sodium trioxonitrate(V);
(ii) copper (II) trioxonitrate (V);
(iii) mercury (II) trioxonitrate (V);
Question 45 Report
(a) Name the gas evolved when dilute hydrochloric acid is added to each of the following solids and the mixture is warmed
(i) sodium trioxocarbonate (IV);
(ii) potassium trioxosulphate (IV);
(iii) iron (II) sulphide.
(b) Name the reagent(s) that you would use to identify the gas in (a)(ii) above.
Question 46 Report
(a) State Le Chatelier's principle
(b) Use Le Chetelier's principle to deduce the conditions that favour a high yield of ammonia in the Haber process
(c) Give the chemical test for ammonia.
(d) State what would be observed when aqueous ammonia solution is added to:
(i) zinc chloride solution, (ii) copper (II) tetraoxosulohate (V) solution
(e) Explain why the H — N — H bond angle in ammonia is less than that of H — C — H in methane
(f) Give two uses of ammonia.
Answer Details
None
Question 47 Report
(a) When is a sample of water said to be hard?
(b) State one difference between temporary and permanent hardness of water
(c) Give one method of removing hardness completely from water
(d) Name two local is used for the production of soap.
