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Question 2 Report
The empirical formula of hydrocarbon containing 0. 12 mole of carbon and 0.36 mole of hydrogen is
Answer Details
Question 4 Report
Which of the following is a waste product in the Solvary Process for the manufacture of sodium trioxocarbonate (IV)?
Answer Details
The Solvay process is a method used to produce sodium trioxocarbonate (IV), also known as sodium bicarbonate or baking soda. In this process, limestone (calcium carbonate) is heated to produce quicklime (calcium oxide), which is then reacted with brine (a solution of sodium chloride) in a reactor vessel called a "Solvay tower." The reaction produces sodium hydroxide and calcium chloride as byproducts. Therefore, the waste product in the Solvay process is calcium chloride.
Question 5 Report
What volume of oxygen will be left unreacted when a mixture of 100cm3 of hydrogen and 200cm,sup>3,/sup> of oxygen are exploded in a eudiometer?
Answer Details
The balanced chemical equation for the reaction between hydrogen and oxygen is: 2H2 + O2 → 2H2O This means that two molecules of hydrogen react with one molecule of oxygen to produce two molecules of water. Using the ideal gas law, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature, we can calculate the number of moles of hydrogen and oxygen present in the mixture before the reaction. Assuming that the pressure and temperature are constant, we have: nH2 = (P * VH2) / (R * T) = (1 atm * 100 cm3) / (0.0821 L atm mol-1 K-1 * 298 K) = 0.00406 mol nO2 = (P * VO2) / (R * T) = (1 atm * 200 cm3) / (0.0821 L atm mol-1 K-1 * 298 K) = 0.00812 mol Since the stoichiometry of the reaction is 2:1 for hydrogen and oxygen, the limiting reactant is hydrogen. This means that all of the hydrogen will react with half of the oxygen to produce water, leaving the other half of the oxygen unreacted. The number of moles of water produced is given by: nH2O = nH2 = 0.00406 mol The number of moles of oxygen consumed is given by: nO2 = nH2 / 2 = 0.00203 mol The number of moles of oxygen left unreacted is given by: nO2 unreacted = nO2 - nO2 consumed = 0.00812 mol - 0.00203 mol = 0.00609 mol Using the ideal gas law again, we can calculate the volume of oxygen left unreacted: VO2 unreacted = (nO2 unreacted * R * T) / P = (0.00609 mol * 0.0821 L atm mol-1 K-1 * 298 K) / 1 atm = 0.150 L = 150 cm3 Therefore, the volume of oxygen left unreacted is 150 cm3.
Question 6 Report
Which of the following is not true of the rusting of iron?
Answer Details
The statement that is not true about the rusting of iron is that "rusting is a reduction process." Rusting is actually an oxidation process, which means that it involves the loss of electrons from the iron atoms in the metal. This loss of electrons causes the iron to become positively charged, which allows it to react with oxygen in the air and water molecules to form hydrated iron oxide, which is the main component of rust. Rusting occurs when iron is exposed to both oxygen and moisture. In the presence of oxygen, iron undergoes a chemical reaction called oxidation, which produces iron oxide or rust. This process is accelerated by the presence of water, which provides the necessary electrons for the reaction to occur more quickly. Rust is typically reddish-brown in color and is composed mainly of hydrated iron (III) oxide, which has the chemical formula Fe2O3•xH2O. The "x" in the formula represents the number of water molecules that can bond to each iron atom in the rust. While rusting may look similar to burning, it is actually a different process. Burning involves a rapid oxidation reaction that produces heat and light, whereas rusting is a slower process that does not produce heat or light.
Question 7 Report
What quantity of silver is deposited when 96500C of electricity is passed through a solution containing silver ions? (Ag = 108, 1F = 96500C)
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Question 8 Report
During the electrolysis of dilute tetraoxosulphate (VI) acid solution 0.05 mole of electrons were passed what volume of gas was produced at the anode? (Gaseous molar volume = 22. 4dm3 at s.t.p)
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Question 9 Report
Which of the following metals cannot extracted from its ore by using carbon (ll) oxide as the reducing agent?
Answer Details
Aluminum (Al) is the metal that cannot be extracted from its ore using carbon (II) oxide as the reducing agent. This is because aluminum is more reactive than carbon and thus cannot be reduced by it. To extract aluminum from its ore, electrolysis is used instead, where the aluminum oxide is dissolved in molten cryolite and a direct current is passed through it, causing the aluminum to be deposited at the cathode. On the other hand, metals like copper (Cu), zinc (Zn), lead (Pb), and iron (Fe) can be extracted from their ores using carbon (II) oxide as the reducing agent because they are less reactive than aluminum and can be reduced by carbon.
Question 10 Report
A salt which loses mass when exposed to air is
Answer Details
The correct answer is "efflorescent". Efflorescence is a process where a salt that contains water molecules loses its water content when exposed to air. The loss of water causes the salt to crumble or turn into a powder, which can result in a decrease in its mass. This occurs because the salt is more soluble in water than in air, and the water molecules in the salt are attracted to the water molecules in the air. As a result, the water molecules in the salt are released into the air, leaving behind the dry salt. This process is commonly observed in some household items like baking soda or washing soda, which can form a white powdery substance on their surface when left exposed to air.
Question 12 Report
Which of the following is not decomposed by heat?
Answer Details
The compound that is not decomposed by heat is sodium carbonate (Na2CO3). When some compounds are heated, they break down into simpler substances. This process is called thermal decomposition. The products of thermal decomposition may include gases, liquids, or solids. Calcium carbonate (CaCO3), copper carbonate (CuCO3), zinc carbonate (ZnCO3), and magnesium carbonate (MgCO3) all decompose when heated to form simpler compounds. For example, when calcium carbonate is heated, it breaks down into calcium oxide (CaO) and carbon dioxide (CO2). However, sodium carbonate (Na2CO3) does not decompose when heated. It is a stable compound that can withstand high temperatures without breaking down. Therefore, it is used in many industrial processes that involve high temperatures, such as glass-making and soap-making. In summary, of the options given, sodium carbonate is the compound that is not decomposed by heat.
Question 14 Report
The reaction represented by the equation NaOH(aq) + HCI(aq) → NaCI(aq) + H2O(/)
Answer Details
The given chemical equation represents a reaction between Sodium Hydroxide (NaOH) and Hydrochloric Acid (HCl) in an aqueous solution. During the reaction, the NaOH reacts with HCl to form Sodium Chloride (NaCl) and water (H2O) as products. The reaction can be represented as follows: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(/) This type of reaction is known as a neutralization reaction as it involves the combination of an acid and a base to form a salt and water. Hence, the correct answer is "is a neutralization". This reaction is not reversible, so the option "is reversible" is incorrect. The reaction does not usually require a catalyst, so the option "is usually catalysed" is also incorrect. Additionally, the option "attains equilibrium after a few seconds" is incorrect as the reaction goes to completion, meaning that all of the reactants will be converted to products, and no reactants will be left.
Question 15 Report
The reaction represented by the equation C(s) + H2O(l) → CO(s) + H 2(s) was carried out at 27oC if the enthalpy change was + 4500 J and the entropy change was + 12J, what was the free energy change? (∆G = ∆H - T∆S)
Question 17 Report
Which of the following does not affect the rate of a chemical reaction?
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Question 18 Report
Which of the following is used as an anaesthetic?
Answer Details
The option that is commonly used as an anaesthetic is CHCI3, which is also known as chloroform. Chloroform is a colorless liquid with a sweet smell, and it was widely used as an anaesthetic in the past. It works by depressing the central nervous system and inducing a state of unconsciousness. However, chloroform has been largely replaced by other anaesthetics due to its potential to cause liver damage and other health problems. Other options, such as C2H5OH or ethanol, may be used for sedation or pain relief but are not typically used as general anaesthetics.
Question 19 Report
Which of the following is not true of the rusting of iron?
Answer Details
The statement that is not true about the rusting of iron is that "rusting is a reduction process." Rusting is an oxidation process, which means that it involves the loss of electrons by iron atoms. When iron reacts with oxygen and water, a redox reaction takes place. Iron atoms lose electrons to oxygen atoms to form iron oxide, while water molecules are split into hydrogen ions and hydroxide ions. The hydrogen ions combine with oxygen atoms to form water molecules, while the hydroxide ions combine with iron ions to form hydrated iron (III) oxide, which is the reddish-brown rust that we see on iron surfaces. Therefore, rusting is not a reduction process but an oxidation process that occurs in the presence of oxygen and moisture. The rust formed is mainly hydrated iron (III) oxide, and the process is similar to corrosion rather than burning.
Question 20 Report
Water gas is a mixture of
Answer Details
Water gas is a mixture of carbon monoxide (CO) and hydrogen gas (H2). It is produced by reacting steam with hot coal or coke in a process known as gasification. The resulting gas mixture is composed of about 50% CO and 50% H2. Water gas has been used historically as a fuel for heating and lighting, and it is still used today in some industrial processes.
Question 21 Report
Which of the following statements is not correct?
Answer Details
The incorrect statement is "Chlorine exhibits allotopy." The correct term is "allotropy," which refers to the ability of an element to exist in different physical forms known as allotropes. Carbon and sulfur are examples of elements that exhibit allotropy. Chlorine, on the other hand, does not exhibit allotropy because it exists only as a gas in its standard state, and does not have any other stable physical forms. Nitrogen is a gas and argon is a noble gas, which means that they do not readily react with other elements.
Question 22 Report
Bubbling of carbon (IV)oxide into calcium hydroxide solution results in the formation of
Answer Details
Bubbling of carbon (IV)oxide into calcium hydroxide solution results in the formation of calcium carbonate (CaCO3). When carbon (IV) oxide gas is bubbled into calcium hydroxide solution, a chemical reaction takes place between them. This reaction is called a precipitation reaction, where a solid is formed from the reaction of two solutions. The chemical equation for the reaction is: Ca(OH)2 + CO2 → CaCO3 + H2O In this reaction, calcium hydroxide (Ca(OH)2) reacts with carbon (IV) oxide (CO2) to form calcium carbonate (CaCO3) and water (H2O). Calcium carbonate is a white solid that is commonly found in nature as a mineral in rocks and shells. It is also used in various applications, such as in the production of cement, as a dietary supplement, and in the manufacturing of paper, plastics, and paint.
Question 23 Report
Given that 32.0g sulphur contains 6.02 x 10 23 sulphur atoms how many atoms are there in 2.70g of aluminium? {Al = 27, S =32}
Answer Details
The given information provides us with the number of atoms present in 32.0g of sulfur, which is 6.02 x 10^23 atoms. Now, we need to find out the number of atoms in 2.70g of aluminum, given that the atomic mass of aluminum is 27. To find the number of atoms in 2.70g of aluminum, we need to first calculate the number of moles of aluminum present in 2.70g. Number of moles = mass/molar mass Molar mass of aluminum = 27g/mol Number of moles of aluminum = 2.70g/27g/mol = 0.1mol Now, we can use Avogadro's number, which is the number of particles (atoms or molecules) in one mole of a substance, to calculate the number of atoms in 0.1mol of aluminum. Avogadro's number = 6.02 x 10^23 particles/mol Number of atoms in 0.1mol of aluminum = 0.1mol x 6.02 x 10^23 particles/mol = 6.02 x 10^22 atoms Therefore, the correct answer is 6.02 x 10^22.
Question 24 Report
The complex salt formed when aluminium dissolves in sodium hydroxide solution is
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Question 25 Report
Which of the following correctly explains why iodine crystals change directly into the gaseous state when heated?
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Iodine crystals change directly into the gaseous state when heated because of a process called sublimation. Sublimation occurs when a solid transitions directly into a gas without first becoming a liquid. Iodine molecules are held together by weak intermolecular forces, which makes it easier for them to break apart and turn into a gas when heated. This process is called sublimation and it explains why iodine crystals can change directly into a gaseous state when heated.
Question 26 Report
Which of the following is not a naturally occurring iron ore?
Answer Details
The naturally occurring iron ores are compounds that contain iron combined with other elements such as oxygen, carbon, and sulfur. Out of the given options, FeCl2 is not a naturally occurring iron ore because it is a compound of iron and chlorine. Iron chloride is not found naturally in the earth's crust as an ore. Fe2O3, Fe2O3O3, FeCO3, and FeS2 are all naturally occurring iron ores. Fe2O3 is commonly known as hematite, Fe2O3O3 is not a known compound, FeCO3 is known as siderite, and FeS2 is known as pyrite or fool's gold.
Question 27 Report
Which of the following does not affect the rate of a chemical reaction?
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Question 28 Report
The main characteristic feature of transition metals is that they
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The main characteristic feature of transition metals is that they have variable oxidation states. This means that they can lose or gain different numbers of electrons when they form chemical compounds, allowing them to have a wide range of chemical properties and reactivities. Transition metals are located in the middle of the periodic table and have partially filled d orbitals, which give rise to their unique properties. Their variable oxidation states also make them important catalysts in many chemical reactions, as they can easily switch between different oxidation states to facilitate reactions.
Question 29 Report
An acid present in proteins is
Answer Details
Among the options given, the acid present in proteins is an amino acid. Proteins are made up of long chains of amino acids linked together, forming a polypeptide chain. Each amino acid has an amine group (-NH2) and a carboxyl group (-COOH). When these groups react with each other, they form a peptide bond, creating a polypeptide chain. Therefore, the acid present in proteins is the carboxyl group of the amino acids, which gives proteins their acidic properties. Other acids listed, such as lactic acid, propanoic acid, palmitic acid, and stearic acid, are not typically found in proteins. Lactic acid is a byproduct of anaerobic respiration in some organisms. Propanoic acid is a naturally occurring acid found in some foods. Palmitic and stearic acids are both saturated fatty acids found in animal fats and some plant oils.
Question 30 Report
Which of the following types of hybridization gives rise to tetrahedral molecules?
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Question 31 Report
Which of the following equations represents the reaction of chlorine with hot concentrated sodium hydroxide solution?
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Question 32 Report
The following are uses of radioactive isotops except for
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Radioactive isotopes are used in various fields, including medicine, research, and industry. They have several unique properties that make them useful for various applications. However, one of the uses of radioactive isotopes is not related to their properties, and that is determining equilibrium positions. Radioactive isotopes can be used for sterilizing medical equipment, tracing reaction paths, dating elements, and radiography. For example, they can be used to kill bacteria, viruses, and other microorganisms that can cause infections in medical equipment. In radiography, they can be used to produce images of internal body parts, which can help diagnose medical conditions. In research, they can be used to trace the path of chemical reactions or determine the age of geological samples. However, determining equilibrium positions is not a common use of radioactive isotopes. Equilibrium positions are typically determined using chemical reactions and thermodynamic principles. Radioactive isotopes can be used to study the kinetics of reactions, but they are not usually used to determine equilibrium positions.
Question 33 Report
Which of the following compound is aromatic?
Answer Details
Benzene is the only compound that is aromatic. Aromaticity refers to a special type of stability in organic molecules that contain a ring of atoms with alternating double bonds. This creates a "delocalized" system of electrons that is spread out over the entire ring, making it particularly stable and resistant to chemical reactions. Benzene has a six-carbon ring with alternating double bonds, making it an aromatic compound. In contrast, cyclobutane, cyclopentane, hexane, and ethene do not have this type of ring and are not considered aromatic. They have different types of bonds and molecular structures that make them less stable and more reactive compared to benzene.
Question 34 Report
Equilibrium is said to be attained in reversible reaction when
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Equilibrium is attained in a reversible reaction when the rates of the forward and backward reactions are equal. This means that the reaction is still ongoing, but the concentrations of the reactants and products have reached a constant state where there is no net change in the concentrations of the reactants and products over time. Think of it like a tug-of-war between the reactants and products. At first, the reactants are winning, and the reaction proceeds in the forward direction, forming products. But as the products build up, they start to pull back in the opposite direction, and the reaction starts to go in reverse. Eventually, the pull from the reactants and products becomes balanced, and the reaction reaches a point where there is no net movement in either direction. So, when the forward and backward rates are equal, the reaction is said to be at equilibrium, and the concentrations of the reactants and products remain constant over time. Note that this does not mean that all the reactants have been used up or all the products have been formed, as the reaction is ongoing but in a state of balance.
Question 35 Report
When copper (ll) chloride solution is treated with excess aqueous ammonia, a deep blue solution results This is due to the presence of
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Question 36 Report
How many isomers can be obtained from C4H10?
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C4H10 is the molecular formula for butane, which is an alkane with four carbon atoms. Isomers are molecules with the same molecular formula but different structural arrangements of their atoms. In the case of butane, there are two main types of isomers: constitutional isomers and stereoisomers. Constitutional isomers have the same molecular formula but different connectivity between atoms. For example, butane has two possible constitutional isomers: n-butane, where the four carbon atoms are arranged in a straight chain, and isobutane, where the carbon atoms form a branched chain. Stereoisomers have the same molecular formula and connectivity between atoms, but differ in the spatial arrangement of their atoms. Butane has no stereoisomers because all of its atoms are connected by single bonds, which do not allow for different spatial arrangements. Therefore, the number of isomers that can be obtained from C4H10 is 2, which correspond to its two constitutional isomers.
Question 37 Report
(a) Explain with equation where appropriate, the functions of the following substances in the Solvay Process:
(i) limestone,
(ii) ammonia,
(iii) brine.
(b) Explain why the reaction between aqueous sodium trioxocarbonate (IV) solution and dilute hydrochloric acid is a neutralization reaction.
(c) Calculate the mass of sodium trioxocarbonate (IV) produced by the complete decomposition of 16.8g of sodium hydrogen trioxocarbonate (IV) (H = 1, O = 16, Na = 23, S = 33)
Answer Details
None
Question 38 Report
(a) How does the collision theory explain the rate of a chemical reaction?
(b) State how each of the following affects the rates of chemical reactions:
(i) surface area (ii) catalyst
Question 39 Report
(a) Explain why transition metals
(i) have high melting points
(ii) have variable oxidation states,
(iii) exhibit paramagnetism
(b) (i) Name the impurities present in bauxite
(ii) State how the impurities in bauxite are removed
(ii) Explain why aluminium oxide is said to be amphoteric.
(c) (i) Describe the electrolysis of copper (II) tetraoxosulphate (VI) solution, using copper electrodes.
(ii) Will the colour of the copper (II) tetraoxosulphate (VI) solution change at the end of the electrolysis described in (c)(i) above? Give reasons for your answer.
Question 40 Report
(a) Give one example of;
(i) heavy chemicals
(ii) fine chemicals
(b) Write the structural formulae and the names of compounds having the formula CH\(_4\)CI,
Question 41 Report
(a) Write the structural formula of:
(i) 2, 2, 4 - trimethylpentane, (ii) ethylmethanoate, (iii) trans 2, 3 - dimethylbut - 2-ene.
(b) Write the structure of the straight-chain compound that is isomeric with 2,2,4 - trimethylpentane.
(c) Write chemical equations to illustrate the oxidation of: (i) a secondary alkanol (ii) a dihydric alkanol.
(d) When-Crushed cassava was warmed with dilute hydrochloric acid, a sweet-tasting compound, D was obtained. When compcund D was treated with the enzyme, zymase and the mixture distilled a clear and colourleCsliduid, E was obtained. When liquid E was warmed with eth anoic acid i n the presence of a few drops of concentrated tetraoxosulphate (V1) acid, a compound F, with fruity smell was obtained
. (i)To what class of compounds does D belong?
(ii) Name E and F
(iii) Write the fun-ctional group in F
(iv) Write the equation for the reaction between E and ethanoic acid in the presence of concentrated tetraoxosulphate (VI) acid.
(v) Name the type of reaction that takes place between E and ethanoic acid.
(e) Arrange the followingcompounds in their correct order of increasing boiling points: CH\(_3\)CH\(_2\)CH\(_2\)OH, CH\(_3\)CH\(_2\)CH\(_2\)CH\(_2\)CH\(_2\)CH\(_3\) and CH\(_2\)CH\(_2\)CH\(_2\)CH\(_3\); Explain the order.
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None
Question 42 Report
(a) Name the major raw materials used in the manufacture of the following:
(i) polythene
(ii) margarine
(iii) cement
(b) State one problem associated with oil producing areas
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None
Question 43 Report
(a) Arrange the following in their correct order of increasing energy: alpha particles, gamma rays and beta particles
(b) State one difference between nuclear fission and nuclear fusion
None
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None
Question 44 Report
(a) Write the ionic equation for the reaction between zinc powder and silver trioxonitrate (VI) solution
(b) Which substance in (a) above is (i) oxidized, (ii) reduced?
(c) State two applications of oxidation numbers
Question 45 Report
(a) An element X is represented as \(^{40}_{20} X\)
(i) How many electrons and how many neutrons are present in the atom of X?
(ii) Write the electronic configuration of the atom
(b) Chlorine, whose atomic number is 17, reacts with the element X to form a compound.
(i) What type of bond is formed between X and chlorine?
(ii) Explain how the bond between X and chlorine is formed
(iii) Write the formula of the compound formed and statelhree properties of the compound.
(c) Chlorine has two isotopes of mass numbers 35 and 37 respectively. Suggest the possible relative molar masses of a chlorine molecule.
(d) Calculate the mass of one atom of carbon, given that one mole of carbon weighs 12.0g. (L = 6.02 x 10\(^{23}\))
Question 46 Report
(a) Name two allotropes of carbon
(b) Name two products of the destructive distillation of coal and state one use of each.
Question 47 Report
(a) What is a carbohydrate?
(b) Name two types of carbohydrates and give one example of each type
Answer Details
None
Question 48 Report
State Gay-Lussac's law and illustrate the law with one chemical reaction.
Question 49 Report
Distinguish between cracking and reforming. Of what importance are the two processes in the petroleum industry?
Question 50 Report
50cm\(^{3}\) of sulphur (IV) oxide were produced at s.t.p. when some quantity of powdered sulphur were burnt in excess oxygen
(a) Write the equation for the reaction
(b) Calculate the volume of oxygen used up during the reaction
(c) Which of the gas laws is applicable? State the law.
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