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Question 1 Report
Calcium atom ionizes by
Answer Details
Calcium atom has 20 electrons in its outermost shell. To attain stability, it needs to lose these electrons. Thus, calcium atom ionizes by losing two electrons to form a calcium ion with a 2+ charge. Therefore, the correct option is "losing two electrons."
Question 3 Report
Which of the following reactions is not feasible?
Answer Details
The reaction that is not feasible is the second one: Cl2 + 2NaF → 2NaCI + F2. This is because fluorine (F2) is a more reactive halogen than chlorine (Cl2), and as such it cannot be displaced from a compound like NaF by chlorine. This is an example of the reactivity series of halogens, where the more reactive halogens displace the less reactive halogens from their compounds.
Question 4 Report
Helium is preferred to hydrogen in filling balloons because hydrogen
Answer Details
Helium is preferred to hydrogen in filling balloons because hydrogen is inflammable. This means that if a balloon filled with hydrogen comes in contact with a flame or spark, it can easily catch fire and explode. On the other hand, helium is non-flammable, making it a safer option for filling balloons.
Question 5 Report
30cm3 pf hydrogen at s.t.p combine with 20cm3 of oxygen to form steam according to the following equation 2H2(g) + O2(g) → 2H2O(g). Calculate the total volume of the gaseous mixture at the end of the reaction
Answer Details
Question 6 Report
An exothermic reaction is one which involves
Answer Details
An exothermic reaction is a chemical reaction that releases energy to the surrounding in the form of heat, light, or sound. This means that in an exothermic reaction, the products have lower energy than the reactants. The energy released during the reaction is given off to the surroundings, which can cause an increase in temperature or a physical change such as a phase change. Therefore, the correct option is "loss of heat to the surrounding".
Question 8 Report
Which of the following is an acid salt?
Answer Details
An acid salt is a salt that contains an acidic ion or proton that can undergo partial hydrolysis in an aqueous solution to form an acidic solution. Among the options given, NaHCO3 is an acid salt because it contains the acidic hydrogen carbonate ion (HCO3-) which can react with water to produce a slightly acidic solution. The other options, NH4CI, MgSO4 7H2O, and CH3COONa, do not contain any acidic ion and therefore are not acid salts.
Question 9 Report
Which of the following is a secondary alkanol?
Answer Details
A secondary alkanol is an alcohol in which the carbon atom bearing the hydroxyl group is bonded to two other carbon atoms. The correct answer is CH3-CH(OH)-CH 3 because the carbon bearing the hydroxyl group (-OH) is bonded to two other carbon atoms.
Question 10 Report
Pauli Exclusion Principle is related to
Answer Details
The Pauli Exclusion Principle is related to the quantum numbers of electrons. It states that no two electrons in an atom can have the same set of four quantum numbers (principal quantum number, azimuthal quantum number, magnetic quantum number, and spin quantum number). This principle is important in determining the electron configuration of atoms and the properties of chemical bonds between atoms. In simple terms, it means that electrons have to occupy different energy levels and different positions within those energy levels in order to form stable atoms and molecules.
Question 11 Report
Which of the following is needed to produce slag during the extraction of iron in the blast furnace?
Answer Details
Limestone is needed to produce slag during the extraction of iron in the blast furnace. The blast furnace is used for extracting iron from its ore, which is a mixture mainly of iron oxide and limestone. When limestone is heated, it decomposes to form calcium oxide (CaO), which then reacts with the impurities in the ore, such as silicon dioxide (SiO2), to form slag. The slag is a waste product that floats on top of the molten iron and is removed from the furnace separately. Therefore, the correct option is B - Limestone.
Question 12 Report
What volume of hydrogen is produced at s.t.p. When 2.60 g of zinc reacts with excess HCI according to the following equation? Zn(s) + 2HCI(aq) → ZnCI 2(aq) + H2(g) [Zn = 65; 1 mole of a gas occupies 22.4dm3 at s.t.p]
Answer Details
The balanced chemical equation is: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) First, we need to find the moles of zinc present: m(Zn) = 2.60 g M(Zn) = 65 g/mol (molar mass of Zn) n(Zn) = m(Zn) / M(Zn) n(Zn) = 2.60 g / 65 g/mol n(Zn) = 0.04 mol According to the balanced equation, 1 mole of zinc reacts with 2 moles of hydrochloric acid to produce 1 mole of hydrogen gas. Since we have an excess of hydrochloric acid, all the zinc will react, and the amount of hydrogen produced can be calculated as follows: n(H2) = n(Zn) × 1 mol H2 / 1 mol Zn n(H2) = 0.04 mol Now we can use the ideal gas law to find the volume of hydrogen produced at STP: PV = nRT where P is the pressure (which is 1 atm at STP), V is the volume, n is the number of moles, R is the gas constant (0.08206 L·atm/mol·K), and T is the temperature (273 K at STP). Solving for V: V = nRT / P V = (0.04 mol) × (0.08206 L·atm/mol·K) × (273 K) / (1 atm) V = 0.89 L V = 0.89 dm3 (since 1 L = 1 dm3) Therefore, the volume of hydrogen produced at STP is 0.89 dm3, which is option (B).
Question 13 Report
In the Periodic Table, the elements that loss electrons most readily belong to
Answer Details
The elements that loss electrons most readily are located in Group 1A, also known as the alkali metals. This is because they have only one electron in their outermost shell, making it easy to remove that electron and form a cation with a positive charge. As we move down the group, the tendency to lose an electron increases due to the decrease in ionization energy. In contrast, the elements in other groups, such as Group VIIA or the halogens, tend to gain electrons to achieve a stable octet configuration, rather than losing them.
Question 14 Report
One mole of a compound M(HCO3)2 has a mass of 162g. Calculate the relative atomic mass of M. [H = 1, C =12, O = 16]
Answer Details
The formula of the given compound is M(HCO3)2. The total mass of the compound is 162g per mole. We need to find the relative atomic mass of M. Let the relative atomic mass of M be x. The molecular weight of the compound will then be: Molecular weight = mass of 1 mole of the compound Molecular weight = 162g/mol The molecular weight can also be calculated as the sum of the atomic weights of all the atoms in the compound. The compound has 2 H atoms, 2 C atoms, and 6 O atoms. Using the atomic weights of H, C, and O as given in the question, we get: Molecular weight = 2x + 2(12) + 6(16) Molecular weight = 2x + 120 + 96 Molecular weight = 2x + 216 We can now equate the two expressions for the molecular weight to get: 2x + 216 = 162 2x = 162 - 216 2x = -54 x = -27 This is a non-sensical value for the relative atomic mass. The reason for this is that we made an error in the calculation. The actual molecular weight of the compound should be: Molecular weight = 2x + 2(1) + 2(12) + 6(16) Molecular weight = 2x + 122 Equating the two expressions for the molecular weight gives: 2x + 122 = 162 2x = 162 - 122 2x = 40 x = 20 Therefore, the relative atomic mass of M is 20. Answer: 40
Question 15 Report
Equal volumes of water were added to one mole of each of the following compounds. Which of them produced the largest number of ions
Answer Details
Question 16 Report
What is the electronic configuration of an element represented as 199X?
Answer Details
Question 17 Report
If an element with high electron affinity combines with another element with low ionization energy the bond formed will be mainly
Answer Details
When an element with high electron affinity combines with another element with low ionization energy, the bond formed will be mainly ionic. This is because the element with high electron affinity has a strong tendency to gain electrons, while the element with low ionization energy has a low energy requirement to lose electrons. When these two elements combine, the element with high electron affinity will take one or more electrons from the element with low ionization energy to achieve a stable electron configuration. This results in the formation of positively and negatively charged ions, which are held together by electrostatic attraction to form an ionic bond. In contrast, covalent bonds involve the sharing of electrons between atoms, dative bonds involve one atom donating both electrons in the bond, and metallic bonds involve a sharing of electrons between many atoms in a metallic lattice. However, none of these types of bonds are likely to be formed when an element with high electron affinity combines with another element with low ionization energy.
Question 18 Report
Alkanoates are produced from alkanols by
Answer Details
Alkanoates are produced from alkanols by esterification. Esterification is a chemical reaction between an alcohol and a carboxylic acid, resulting in the formation of an ester and water. In this case, an alkanol (an alcohol with a carbon chain) reacts with a carboxylic acid to form an alkanoate (an ester with a carbon chain) and water. This process involves the removal of a hydroxyl (-OH) group from the alcohol and a hydrogen atom from the carboxylic acid, which then combine to form water. The remaining portions of the alcohol and carboxylic acid combine to form the ester (alkanoate).
Question 19 Report
Which of the following compounds reacts with sodium hydroxide to form a salt?
Answer Details
Question 20 Report
When dilute copper (ll) chloride solution is electrolysed, the reaction at the cathode is represented by the equation
Answer Details
The reaction at the cathode during electrolysis of dilute copper (II) chloride solution can be determined by analyzing the oxidation states of the species involved. In the electrolysis of copper (II) chloride solution, the positive copper ions (Cu2+) migrate towards the cathode (negatively charged electrode), where they gain electrons and are reduced to form copper atoms (Cu). Therefore, the equation representing the reaction at the cathode is: Cu2+ + 2e- → Cu Option (ii) represents this equation and is the correct answer.
Question 21 Report
Which of the following movements can be described as random motion?
Answer Details
Gas molecules colliding in a flask can be described as random motion. When gas molecules are in motion, they collide with each other and the walls of the container in which they are enclosed. The motion of these gas molecules is completely random, and they move in different directions at different speeds. The kinetic energy of the gas molecules determines the speed and motion of the molecules. Therefore, the random motion of gas molecules is a consequence of their kinetic energy. On the other hand, the wheelbarrow being pushed, car travelling on a straight line, and planets going around the sun follow specific trajectories and patterns. They move in a specific direction and are influenced by forces acting upon them. Thus, these movements are not considered random motion.
Question 22 Report
Which of the following is the most reactive towards bromine?
Answer Details
Bromine is a halogen, which means it has a high electronegativity and is very reactive towards compounds with lower electronegativities. In this case, we are looking for the compound that is most likely to react with bromine. Methane, benzene, ethyne, and hexane are all hydrocarbons, which means they are composed of hydrogen and carbon atoms. However, they differ in their chemical structures and properties. Out of these options, ethyne (also known as acetylene) is the most reactive towards bromine. This is because it has a triple bond between its two carbon atoms, which makes it more susceptible to reactions with other compounds. The triple bond is composed of two pi bonds and one sigma bond, and the pi bonds are more easily broken, allowing ethyne to react with bromine more readily. In contrast, methane and hexane have only single bonds between their carbon atoms, which makes them less reactive towards bromine. Benzene has a delocalized ring of electrons, which makes it more stable and less likely to react with other compounds, including bromine.
Question 23 Report
What will be the effect of increase in pressure on the following system at equilibrium? 2NH2(g) N2(g) + 3H2(g)
Question 24 Report
Which of the following compounds dissolves in water to form a solution with pH below 7?
Answer Details
Among the given options, the only compound that dissolves in water to form a solution with pH below 7 is ammonium chloride (NH4Cl). When NH4Cl is dissolved in water, it dissociates into ammonium ions (NH4+) and chloride ions (Cl-). The ammonium ion, NH4+, is the conjugate acid of a weak base (NH3), and it reacts with water to form hydronium ions (H3O+). This reaction produces an acidic solution with a pH below 7. On the other hand, sodium tetraoxosulphate (VI) (Na2SO4), potassium hydroxide (KOH), and sodium trioxocarbonate (IV) (Na2CO3) are all basic compounds. When they are dissolved in water, they dissociate to form hydroxide ions (OH-) which react with water to form hydroxide ions (OH-) and hydronium ions (H3O+). This reaction produces an alkaline solution with a pH greater than 7.
Question 25 Report
How many carbon atoms are present in one molecule of 2-methylpropane?
Answer Details
The chemical formula for 2-methylpropane is C4H10, which means it has four carbon atoms. Therefore, the answer is 4.
Question 26 Report
Which of the following atoms contains the highest number of electrons in the outermost shell?
Answer Details
Question 27 Report
Which of the following lowers the activation energy of a chemical reaction?
Answer Details
A catalyst is a substance that lowers the activation energy of a chemical reaction, which means it makes it easier for the reactants to reach the transition state and form products. This is achieved by providing an alternative reaction pathway that has a lower activation energy. Catalysts are not consumed during the reaction and can be used repeatedly. The other options, freezing mixture, reducing agent, and water, do not lower the activation energy of a chemical reaction.
Question 28 Report
Which of the following halogens is the most reactive?
Answer Details
Fluorine (F2) is the most reactive of the halogens. This is because of its small atomic size and high electronegativity, which allows it to attract electrons easily and form strong bonds with other elements. Additionally, the F-F bond is very weak, which means that it is relatively easy to break and form new compounds. As a result, fluorine reacts vigorously with most other elements, including metals and non-metals.
Question 29 Report
Environmental pollution problems are generally more severe in countries which have
Answer Details
Environmental pollution problems are generally more severe in countries which have a dense population. This is because a dense population means there are more people living in a smaller area, leading to higher levels of waste generation, energy consumption, and transportation needs. As a result, the pollution levels tend to be higher due to increased industrialization and use of resources. In addition, the higher population density also leads to increased competition for resources such as land, water, and food, which can also contribute to environmental degradation.
Question 30 Report
Exhaust fumes discharged from a smoky vehicle gradually become invisible as a result of
Question 31 Report
Which of the following is not correct about oxidation number convention? The oxidation number of a/an
Answer Details
The statement that is not correct about the oxidation number convention is "atom of a diatomic molecule is +2". The oxidation number of an atom in a diatomic molecule depends on the molecule, and can be either positive, negative or zero. For example, in the diatomic molecule HCl, the oxidation number of H is +1 and the oxidation number of Cl is -1. In the diatomic molecule O2, the oxidation number of each O atom is 0. Therefore, the correct answer is "atom of a diatomic molecule is +2"
Question 32 Report
Which of the following properties increases down a group in the Periodic Table?
Answer Details
The property that increases down a group in the Periodic Table is atomic radius. Atomic radius is the distance between the nucleus of an atom and its valence electrons, which determines the size of the atom. As one goes down a group in the periodic table, the number of energy levels (shells) in the atom increases, making the atomic radius larger. This is due to the increasing distance between the nucleus and valence electrons as the number of shells increases. Therefore, the correct option is atomic radius.
Question 33 Report
Which of the orbitals 4s, 4p, 4d and 4f has the lowest energy?
Answer Details
The energy of an electron in an atom is determined by its orbital. The orbitals with the lowest energy are filled first before the higher energy orbitals. The order of filling of orbitals is governed by Aufbau principle, which states that electrons fill the lowest energy orbital available before occupying higher energy orbitals. Based on this principle, the 4s orbital has the lowest energy among the given options, followed by 4p, 4d, and 4f in increasing order of energy. Therefore, the 4s orbital has the lowest energy. So, the answer is 4s.
Question 34 Report
Which of the following compounds is unsaturated?
Answer Details
Out of the given options, the compound that is unsaturated is Methylbenzene. This is because the term "unsaturated" refers to a compound that contains at least one carbon-carbon double or triple bond. Methylbenzene, also known as toluene, has a double bond between one of its carbon atoms and the adjacent carbon atom in the benzene ring. Therefore, it is an unsaturated compound. The other options, 2-methylbutane, chloromethane, and 1,2-dibromoethane, are all saturated compounds as they contain only single bonds between their carbon atoms.
Question 35 Report
Gas molecules are said to be perfectly elastic because
Answer Details
Gas molecules are said to be perfectly elastic because they collide without loss of energy. When gas molecules collide with each other, they exchange energy and momentum, but the total energy and momentum of the molecules remain constant. This is due to the fact that gas molecules are very small and have negligible attractive forces between them. As a result, they are able to move about freely in straight lines and collide with each other in a perfectly elastic manner, without any loss of energy. Therefore, when gas molecules collide, they bounce off each other with the same energy that they had before the collision. This property of gas molecules is known as perfect elasticity, which is a key characteristic of gases.
Question 36 Report
Equal volumes of CO2 cnd CO at s.t.p have the same
Answer Details
Equal volumes of CO2 and CO at s.t.p have the same number of molecules. This is because at s.t.p, which stands for standard temperature and pressure (0 degrees Celsius and 1 atm pressure), gases occupy the same volume when they contain the same number of molecules. The molar volume of any gas at s.t.p is 22.4 liters, regardless of the gas's mass or density. Therefore, equal volumes of CO2 and CO at s.t.p will contain the same number of molecules.
Question 37 Report
Geometric (cis-trans) isomerism is exhibited by
Question 38 Report
Consider the reaction represented by the following equation: H2(g) + 12(g) → 2HI(g). The number of effective collisions of molecules of the reactants decreases as
Answer Details
The number of effective collisions of molecules of the reactants decreases as the volume of the system is increased. As the volume of the system increases, the space available for the molecules to collide with each other decreases. This leads to a decrease in the frequency of collisions, which in turn decreases the number of effective collisions. Effective collisions are those collisions between reactant molecules that have enough energy and correct orientation to lead to the formation of products. When the volume of the system is increased, the number of collisions decreases, and therefore the number of effective collisions also decreases.
Question 39 Report
Two radioactive elements Q and S have half-life periods of 10 hours and 20 hours respectively. Therefore
Question 40 Report
The greenhouse effect is a climatic condition associated with the presence of excess
Answer Details
The greenhouse effect is a climatic condition associated with the presence of excess carbon (IV) oxide. When certain gases such as carbon dioxide, methane, and water vapor accumulate in the Earth's atmosphere, they trap heat from the sun and prevent it from escaping into space. This trapped heat then warms the planet's surface and leads to the greenhouse effect, which can cause significant changes to the Earth's climate and weather patterns. Carbon dioxide is the most important of these greenhouse gases, and its increasing concentration in the atmosphere due to human activities such as burning fossil fuels is a major contributor to global warming and climate change.
Question 41 Report
The property of calcium chloride which makes it useful as a drying agent is that it is
Answer Details
Calcium chloride is a deliquescent salt, which means it can absorb moisture from the air and turn into a liquid. This property makes it useful as a drying agent because it can remove moisture from the surroundings and keep the environment dry. When calcium chloride is added to a container with a moist substance, it absorbs the moisture and forms a liquid solution. This makes it effective in preventing the formation of rust, as well as in the drying of gases and solvents. Therefore, the correct answer is "deliquescent".
Question 42 Report
If the solubility of KHCO3 is 0.40 mole dm-3 at room temperature , calculate the mass of KHCO3 in 100dm3 of the solution at this temperature. [KHCO3 = 100hmol]
Answer Details
Question 43 Report
(a)(i) State three postulates of the kinetic theory of gases.
(ii) Draw a sketch to illustrate Boyle's law.
(iii) Explain what is meant by "absolute zero of temperature".
(b) Equal volumes of a gas X and oxygen are at the same pressure but temperature of 200 K and 800K respectively.
(i) Giving reason for your answer, state which of the gas samples contains the greater number of molecules.
(ii) If the mass of one molecule of the gas X is 2.19 x 10\(^{-22}\) g, determine the molar mass of X. [Avogadro constant = 6.02 x 10\(^{-23}\)]
(iii) Hence, state with reason which of X and oxygen will diffuse faster under the same conditions. [O= 16].
(c)(i) Mention two reaction conditions that can increase the yield of ammonia in the reaction represented by the following equation: N\(_{2(g)}\) + 3H\(_{2(9)}\) \(\rightleftharpoons\) 2NH\(_{3(g)}\) \(\Dellta\)H = -46kJmol\(^{-1}\). Draw a labelled energy profile diagram for an endothermic reaction.
(iii) A solid W decomposes on heating according to the following equation: W\(_{(s)} \to Y_{(s}) + Z_{(g)}\) List two factors apart from temperature, which can affect the rate of the reaction.
Question 44 Report
(a)(i) Give two differences between a conductor and an electrolyte.
(ii) State three applications of electrolysis.
(iii) Write equation for the reaction at each electrode when a dilute solution of sodium chloride is electrolysed using carbon electrodes.
(b)(i) What is an electrochemical cell?
(ii) Give two examples of primary cells.
(iii) Split the following equation into two balanced hall cell equations. Mte + Fe\(^{2+} \to Mg^{2+} + Fe\).
(c)(i) A current of 0.72 amperes was passed through dilute tetraoxosulphate (VI) acid for 3 hours 20 minutes. Calculate the quantity of electricity that was passed
(ii) If 1 dm\(^3\) of gas evolved at the cathode during the electrolysis of acidified water, what was the volume of gas evolved at the anode?
(d)(i) 20g of copper(II) oxide was warmed with 0.05 mole of tetraoxosulphate (VI) acid. Calculate the mass of copper (II) oxide that was in excess. The equation for the reaction: CuO\(_{(s)}\) + H\(_2\)SO\(_{4(aq)}\) ---> CuSO\(_{4(aq)}\) + H\(_2\)O\(_l\) [0 = 16 ; Cu = 64]
(ii) What type of reaction was involved in (d)(i)?
Question 45 Report
(a)(i) List two elements which react with steam at red heat to produce hydrogen.
(ii) Explain why an aqueous solution of potassium bromide turned reddish brown on bubbling chlorine through it.
(iii) Write an equation for the reaction in (a)(ii).
(b)(i) Name two types of chemical industry that use limestone as raw material.
(ii) Give one example of hygroscopic substances.
(iii) Copy and complete the table below.
| Salt to be prepared |
Starting material | Method of preparation |
| PbSO\(4\) | Pb(NO\(_3)_{2(ag)}\) | - |
| KNO\(_3\) | KOH | Neutralization |
| CaCl\(_2\) | CaCO\(_3\) | - |
| FeCl\(_3\) | Fe\(_(s)}\) | - |
| CuSO\(_4\) | CuO | - |
(c) In the contact process for the manufacture of tetraoxosulphate (VI) acid;
(i) State how sulphur (IV) oxide is obtained;
(ii) Write an equation for the reaction that takes place in the catalyst chamber;
(iii) Give the steps required to convert sulphur (VI) oxide to acid.
(d)(i) List two disadvantages of hard water.
(ii) Mention three methods which can be used to remove both permanent and temporary hardness in water at the same time.
(iii) State the role of alum and chlorine respectively in the purification of water for town supply.
Answer Details
None
Question 46 Report
(a)(i) Define allotropy.
(ii) Name the allotrope of carbon used in gas masks.
(iii) Mention two other elements which exhibit allotropy apart from carbon.
(b) List the products of each of the following reactions:
(i) Heating coal in the absence of air.
(ii) Burning of candle wax in plentiful supply of air
(c)(i) State the two properties of carbon (IV) oxide which make it useful in extinguishing fire.
(ii) Write an equation for the reaction of carbon (IV) oxide with lime water
(iii) Calculate the volume of oxygen that was in excess if 150cm\(^3\) of carbon (II) oxide was burnt in 80cm\(^3\) of oxygen according to the following equation: 2CO\(_{(g)}\) + O\(_{2(g)}\) \(\to\) 2CO\(_{2(g)}\).
(d)(i) State how nitrogen can be obtained from ammonia gas.
(ii) Name the gaseous fuels obtained when steam and air are passed over red hot coke.
(iii) Which of the fuels in (d)(ii) has the lower heating ability? Give reason for your answer.
None
Answer Details
None
Question 47 Report
a)(i) State three differences between covalent compounds and electrovalent compounds.
(ii) Two elements represented as K and L have atomic numbers of 12 and 8 respectively. Write their electronic structures and state the group to which each belongs in the Periodic Table.
(iii) If an alkali metal M exists naturally as the oxide, state with reason whether or not M can be extracted by reduction of the oxide with coke.
(b)(i) What is meant by the half-life of a radioactive element?
(ii) Mention the radioactive isotope used in dating archaeological specimens.
(iii) Balance the following equation and identify Q,
\(^{28}_{13}Al\) —> \(^{24}_{13}Si + \(^{0_1Q\)
(c)(i). Give three chemical properties of metals.
(ii) State two reasons why duralumin preferred to steel in aircraft manufacture.
(iii) What term is used to describe the ability of metals to be hammered into thin sheets?
(iv) Calculate the number of mole of electrons involved in the oxidation of 2.8g of iron filings to iron (II) ions. [Fe = 56].
Answer Details
None
Question 48 Report
(a) The letters R,S,T represent an alkene, an alkene and a terminal alkyne respectively. Which of R, S and T typically undergo(es) the following reactions?
(i) Addition reaction;
(ii) Combustion;
(iii) Substitution reaction.
(b)(i) Name the process by which an alkanol can be converted to an alkene.
(ii) Write the name and structural formula of the third member cf the alkanol series.
(iii) State what would be obtained if a primary alkanol reacted with excess acidified KMnO\(_4\) solution.
(c)(i) Give one chemical test for alkanoic acids.
(ii) Write an equation to show how methanoic acid reacts with ethanol in the presence of mineral acids.
(iii) What is the role of mineral acid in the reaction in (c) ii?
(d) In an experiment, cassava was pressure-cooked to release starch granules, followed by treatment with malt for about 2 hours at 55°C. Yeast was then added and the mixture was left for 2 days at 27°C. An organic product J and a gas H were obtained.
(i) Identify H
(ii) State the class of carbohydrates to which starch belongs and explain what happened to the starch during treatment with malt.
(iii) Draw a labelled diagram of a suitable set-up for obtaining a sample of J from the reaction mixture.
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