WAEC SSCE - Chemistry - 2016

An unsaturated solution differs from a saturated solution at a given temperature because it

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An unsaturated solution differs from a saturated solution at a given temperature because it can still dissolve more solute at that temperature, while a saturated solution has already dissolved the maximum amount of solute that it can hold at that temperature. Therefore, an unsaturated solution has a lower concentration of solute compared to a saturated solution. The ability of a solution to dissolve more solute depends on the nature of the solute, the solvent, and the temperature of the solution.

When element \(_{20}\)Y combines with element \(_8\)Z, it forms

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The answer to the question depends on the electronic configuration and reactivity of the elements Y and Z. Element Y has an atomic number of 20, indicating it has 20 protons in its nucleus, while element Z has an atomic number of 8, indicating it has 8 protons in its nucleus. To determine the type of compound formed, we need to consider the electronegativity of each element. Electronegativity is the measure of an atom's ability to attract electrons towards itself when it forms a chemical bond. Generally, when elements with a large difference in electronegativity combine, they form an ionic compound, while elements with similar electronegativity combine to form covalent compounds. Since Y has a larger atomic number than Z, it has more electrons in its valence shell, making it less electronegative than Z. Therefore, Y is more likely to donate its electrons to Z, forming an ionic compound with the formula YZ. So, the correct option is "An ionic compound, YZ is formed."

Which of the following bonds are broken when ethanol is boiled?

I. Covalent bonds
II. Ionic bonds
III. Hydrogen bonds

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The correct answer is III only - hydrogen bonds are broken when ethanol is boiled. Ethanol is a molecule that contains both polar and nonpolar regions due to the presence of the hydroxyl (-OH) group. The polar region of ethanol allows it to form hydrogen bonds with neighboring ethanol molecules. These hydrogen bonds are relatively weak and require less energy to break than covalent or ionic bonds. When ethanol is boiled, the increased thermal energy breaks the hydrogen bonds between the ethanol molecules, allowing the molecules to escape into the gas phase. The covalent bonds within the ethanol molecules and the ionic bonds between any ions present in the solution are not affected by boiling and remain intact.

Which of the following sources of energy contributes to green-house effect?

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Natural gas contributes to the greenhouse effect. When natural gas is burned, it produces carbon dioxide (CO2), which is a greenhouse gas that contributes to global warming. The combustion of natural gas also releases small amounts of other greenhouse gases, such as methane. Methane is a potent greenhouse gas that is about 25 times more effective at trapping heat than carbon dioxide over a 100-year time span. Therefore, the use of natural gas as a source of energy contributes to the greenhouse effect.

The pH of four solutions M,N,Q and R are 2,6,8 and 11 respectively.
Which of the following deductions about the solutions is correct?

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Which of the following factors will affect the rate of the reaction represented by the following equation?
2HCl(aq) + CaCO3(s) \(\rightarrow\) CaCl2(aq) + H2O(1) + CO2(g)

I. Pressure
II.Concentration
III. Nature of reactants
IV. Temperature

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Propane carbon(IV)oxide diffuse at the same rate because [H = 1.00, C = 12.0, O = 16.0]

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The diffusion rate of a gas is directly proportional to its molecular mass. Propane (C3H8) has a higher molecular mass than carbon dioxide (CO2). However, since the question asks about carbon(IV)oxide (CO2), which has a molecular mass of 44, the answer is that propane and carbon(IV)oxide diffuse at the same rate because they have the same relative molecular mass. Therefore, "They have the same relative molecular mass" is the correct answer.

An aqueous solution of (NH4)2 SO4 is

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An aqueous solution of (NH4)2SO4 is acidic. When ammonium sulfate ((NH4)2SO4) is dissolved in water, it dissociates into its ions: 2 NH4+ and SO4 2-. The ammonium ion (NH4+) is a weak acid and tends to donate a hydrogen ion (H+) to the water molecules, resulting in the formation of hydronium ions (H3O+). This increases the concentration of H+ ions in the solution and makes it acidic. The chemical equation for the dissociation of ammonium sulfate in water is as follows: (NH4)2SO4 + H2O → 2 NH4+ + SO4 2- + H2O Therefore, among the options provided, the correct answer is acidic.

Consider the following half-cell reactions.
Al_(s) \(\to\) Al³⁺_(aq) + 3e^-
Cu²⁺_(aq) + 2e^- \(\to\) Cu_(s)

The overall equation for the reaction is

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How many electron are present in 94Be2+?

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Beryllium has 4 electrons and a 2+ ion means it has lost 2 electrons. Therefore, the number of electrons present in 94Be2+ ion can be calculated by subtracting 2 from the original number of electrons in beryllium. Thus, the number of electrons in 94Be2+ ion is 2. Therefore, the answer is (a) 2.

Which of the following substances is a non-electrolyte?

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A non-electrolyte is a substance that does not conduct electricity when dissolved in water. It is usually a covalent compound that does not dissociate into ions when dissolved in water. Among the given substances, only C₆H₁₂O₆ (glucose) is a non-electrolyte because it is a covalent compound made up of molecules that do not dissociate into ions in water. The other substances are electrolytes because they either ionize or dissociate into ions in water and conduct electricity. H₂SO₄ and NH₄Cl are strong electrolytes because they dissociate completely into ions in water, while CH₃COOH is a weak electrolyte because it only partially ionizes in water.

The boiling points of HF, H2O and NH3 increase in the order of

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The boiling point of a substance is the temperature at which it changes its state from liquid to gas. The boiling point of a substance is dependent on its intermolecular forces, which include van der Waals forces, hydrogen bonding, and dipole-dipole interactions. The stronger the intermolecular forces, the higher the boiling point. In the given options, NH₃, H₂O, and HF are all polar molecules, which exhibit hydrogen bonding, the strongest of intermolecular forces. Among the given options, HF molecules have the strongest hydrogen bonding as compared to H₂O and NH₃ molecules. Therefore, HF has the highest boiling point among the given options. Similarly, NH₃ molecules have the weakest hydrogen bonding as compared to HF and H₂O molecules, so NH₃ has the lowest boiling point among the given options. Therefore, the order of increasing boiling points is NH₃ < HF < H₂O. Hence, the correct option is: "NH₃ < HF < H₂O".

Which of the following apparatus can be used to measure a specific volume of a liquid accurately?

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Out of the given options, the apparatus that can be used to measure a specific volume of a liquid accurately is a pipette. A pipette is a glass or plastic tube that is used to transfer a measured volume of liquid from one container to another. It is designed to dispense a very precise volume of liquid, typically ranging from 1 to 100 milliliters, depending on the type of pipette. Pipettes are often used in chemistry and biology experiments where precise measurements of liquid volumes are critical to the success of the experiment. Beakers and conical flasks can hold liquids but are not designed for accurate measurement of volumes. A measuring cylinder can measure volumes, but it may not be as precise as a pipette.

When a compound X is heated with concentrated tetraoxosulphate(VI)acid, it produces an alkene. X ia an

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Consider the following ionic equation:
Cr₂O₇^2- + 14H⁺ + ne^- \(\to\) 2Cr³⁺ + 7H₂O.
The value of n in the equation is_______?

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Chemicals that are produced in small quantities and with very degree of purity are

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Chemicals that are produced in small quantities and with a very high degree of purity are called "fine chemicals". Fine chemicals are also known as "specialty chemicals" or "performance chemicals". They are typically produced in relatively small quantities (usually less than 1000 tons per year) and are used for specific purposes in industries such as pharmaceuticals, biotechnology, agrochemicals, and electronics. Fine chemicals are produced through complex and highly specialized processes that require a high degree of technical expertise and advanced manufacturing techniques. The production of fine chemicals requires strict control of the purity and quality of the raw materials, as well as the process conditions, in order to ensure that the final product meets the required specifications and standards. Overall, the production of fine chemicals requires a high level of skill and expertise, and is often carried out by specialized companies that focus on producing these highly specialized chemicals.

Consider the following reaction equation
C₂H_4(g) + 3O_2(g) \(\to\) 2CO_2(g) + 2H₂O_(l).

The volume of oxygen at s.t.p that will be required to burn 14g of ethene is
[C₂H₄ = 28; Molar volume of gas at s.t.p = 22.4dm³

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To solve this problem, we need to first balance the chemical equation: C₂H_4(g) + 3O_2(g) → 2CO_2(g) + 2H₂O_(l)
From the balanced equation, we can see that 1 mole of ethene reacts with 3 moles of oxygen gas to produce 2 moles of carbon dioxide gas and 2 moles of liquid water.
We can calculate the number of moles of ethene using the given mass and molar mass: n(C₂H₄) = m/M = 14/28 = 0.5 moles
Using the mole ratio from the balanced equation, we can calculate the number of moles of oxygen required: n(O₂) = 3n(C₂H₄) = 1.5 moles
Finally, we can use the ideal gas law to calculate the volume of oxygen at s.t.p: PV = nRT V = nRT/P = (1.5 mol)(8.31 J/mol K)(273 K)/(101,325 Pa) = 33.6 dm³
Therefore, the volume of oxygen at s.t.p that will be required to burn 14g of ethene is 33.6 dm³.
Answer: 33.6dm³.

Which of the following metals is common to both brass and bronze?

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Copper is the metal that is common to both brass and bronze. Brass is an alloy made of copper and zinc, while bronze is an alloy made of copper and tin. Since copper is a primary component of both alloys, it is the metal that is common to both brass and bronze.

The refreshing characteristic taste of fizzy drinks is due ot the presence of

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Ripening of fruits is hastened by using

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The ripening of fruits is hastened by using ethene. Ethene is a plant hormone that regulates the process of ripening in fruits. It is produced naturally by plants, including fruits, and can also be produced synthetically. When ethene gas is introduced to a fruit, it triggers a series of biochemical reactions that lead to the ripening of the fruit. The gas promotes the breakdown of chlorophyll, which gives fruits their green color, and the conversion of starches into sugars. This process makes the fruit softer and sweeter, and also stimulates the production of more ethene gas, which in turn hastens the ripening of the fruit.

A compound with molecular formula CH₂O₂ is

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Which of the following compounds is/are secondary alkanols?

i) CH₃CH(CH₃)CH₃OH
ii) CH₃CH₂CH(OH)CH₃
iii) CH₃C(OH)(CH₃)CH₃

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Which of the following salts when dissolved in water will form a solution that will change blue litmus to red?

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The salt that will change blue litmus to red when dissolved in water is NH₄Cl. This is because NH₄Cl undergoes hydrolysis in water to form NH₄OH and HCl. NH₄OH is a weak base and will react with water to produce NH₄⁺ and OH^- ions. The OH^- ions will increase the concentration of hydroxide ions in the solution, making it slightly basic. Litmus paper is an indicator that changes color in response to the pH of a solution. Blue litmus paper turns red in acidic solutions, and since the NH₄Cl solution is slightly basic, it will change the blue litmus paper to red.

When NH₄Cl_(s) is dissolved in water, the container feels cold to touch. This implies

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When NH₄Cl_(s) is dissolved in water, the container feels cold to touch, indicating that the process is endothermic. Endothermic processes absorb energy from the surroundings to proceed. In this case, the dissolution of NH₄Cl in water requires energy to break the ionic bonds between the NH₄⁺ and Cl^- ions in the solid and to separate the water molecules from each other. This energy is absorbed from the surroundings, causing the container to feel cold to the touch. The formation of a saturated solution or the solubility of NH₄Cl in water is not indicated by the cooling effect.

The energy which accompanies the addition of an electron to an isolated gaseous atom is

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The energy which accompanies the addition of an electron to an isolated gaseous atom is called electron affinity. When an atom gains an electron, it becomes a negatively charged ion. The energy released or absorbed when this process occurs is the electron affinity. If energy is released when an electron is added to the atom, then the electron affinity is negative, and if energy is absorbed, then the electron affinity is positive. Therefore, the correct option is "electron affinity."

How many moles of oxygen would contain 1.204 x 10²⁴ molecules?
[Avogadro's constant (NA) = 6.02 x 10²³]

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To determine the number of moles of oxygen, we need to use Avogadro's constant, which is the number of particles in one mole of a substance. Given that the number of oxygen molecules is 1.204 x 10^24, we can use this information to calculate the number of moles of oxygen using the following formula: Number of moles = Number of particles / Avogadro's constant Plugging in the values, we get: Number of moles = 1.204 x 10^24 / 6.02 x 10^23 Number of moles = 2 Therefore, the answer is 2. Hence, is the correct answer.

Aluminium is used in the manufacture or aircraft because it

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Aluminium is used in the manufacture of aircraft because it is light and resists corrosion. Aircraft need to be as light as possible in order to fly efficiently, and aluminium is a lightweight metal. Additionally, aluminium naturally forms a layer of oxide on its surface which protects it from further corrosion, making it an ideal material for use in aircraft which are exposed to harsh environmental conditions.

The spreading of the scent of a flower in a garden is an example of_____?

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The spreading of the scent of a flower in a garden is an example of diffusion. Diffusion is the movement of particles (molecules, ions or atoms) from an area of higher concentration to an area of lower concentration. In this case, the scent molecules of the flower move from the area of high concentration (the flower) to an area of lower concentration (the surrounding air) until they are evenly distributed throughout the space. This spreading of the scent is an example of the random movement of particles due to diffusion.

An atom X consist of 6 protons, 6 electrons and 7 neutrons. Which of the following representations of the atom is correct?

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An element X froms the following oxides X₂O, XO and XO₂. This phenomenon illustrates the law of________?

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The phenomenon illustrated in this question is the law of multiple proportion. According to this law, when two elements combine to form more than one compound, the different masses of one element that combine with a fixed mass of the other element are in the ratio of small whole numbers. In the given example, element X combines with oxygen to form three different oxides, and the ratios of the masses of X to oxygen in these oxides are in the ratio of small whole numbers (2:1, 1:1, and 1:2). This is consistent with the law of multiple proportion, which states that when two elements (in this case, X and oxygen) form more than one compound, the ratios of the masses of one element (X) that combine with a fixed mass of the other element (oxygen) are in the ratio of small whole numbers.

The mass of potassium hydroxide required to make 300.ocm³ of 0.4 moldm^-3 solution is {KOH = 56.0}

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To calculate the mass of potassium hydroxide required, we can use the formula: mass = moles × molar mass First, let's calculate the number of moles of potassium hydroxide required to make 300 cm³ of 0.4 mol dm^-3 solution: moles = concentration × volume moles = 0.4 mol dm^-3 × 0.3 dm³ = 0.12 moles The molar mass of potassium hydroxide (KOH) is 56.0 g mol^-1, so we can now calculate the mass of KOH required: mass = moles × molar mass mass = 0.12 moles × 56.0 g mol^-1 = 6.72 g Therefore, the mass of potassium hydroxide required to make 300 cm³ of 0.4 mol dm^-3 solution is 6.72 g. So, the correct option is (C) 6.72g.

The minimum amount of energy required for effective collisions between reacting particles is known as

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Activation energy is the minimum amount of energy required for effective collisions between reacting particles. In a chemical reaction, reactant molecules must collide with a certain minimum amount of kinetic energy in order for the reaction to occur. The reactant molecules must also collide with the correct orientation in order for the reaction to take place. The minimum amount of energy required for these effective collisions is known as the activation energy. Activation energy is a barrier that must be overcome for a reaction to occur. This barrier can be overcome by increasing the temperature of the reaction, since this increases the kinetic energy of the reactant molecules, making them more likely to collide with sufficient energy to react. Alternatively, a catalyst can be used to lower the activation energy barrier and increase the rate of the reaction. In summary, the correct option in the question is activation energy, which is the minimum amount of energy required for effective collisions between reacting particles.

The shape of the water molecule is_______?

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The shape of the water molecule is V-shaped. The water molecule has two hydrogen atoms and one oxygen atom, and the three atoms are not in a straight line, but form a V-shape. This is because of the arrangement of the electron pairs in the molecule. The two lone pairs of electrons on the oxygen atom repel the two hydrogen atoms, pushing them down and creating a V-shape. This shape gives water many of its unique properties, such as its ability to form hydrogen bonds and its high surface tension.

A consequences of global warming is

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The bond formed between H₂O and H₊ to form the hydroxonium H₃O₊ is

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Which of the following elements would produce coloured ion in agueous solution?

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Copper is the element that would produce a colored ion in aqueous solution. Copper ions have a tendency to form complex ions with water or other molecules, which can result in a range of colors depending on the specific ligands involved. For example, copper(II) sulfate forms a blue-colored solution when dissolved in water, while copper(II) chloride forms a green-colored solution. In general, transition metals such as copper are more likely to produce colored ions in solution due to the presence of unpaired electrons in their d orbitals.

The oxidation number of sulphur is +4 in

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The oxidation number of an atom is a measure of the number of electrons it has gained or lost, assuming that the electrons in a chemical bond are assigned to the more electronegative atom. In the compound H₂SO₃, there are two hydrogen atoms, each with an oxidation number of +1, and one oxygen atom, which has an oxidation number of -2. The sum of the oxidation numbers in H₂SO₃ is zero, since the compound is neutral. Therefore, we can calculate the oxidation number of sulfur as follows: 2(+1) + x + 3(-2) = 0 Solving for x, we get: x = +4 Therefore, the oxidation number of sulfur in H₂SO₃ is +4. In summary, the correct option in the question is H₂SO₃, where the oxidation number of sulfur is +4.

The following atoms of carbon ¹²₆C, ¹³₆C and ¹⁴₆C can be described as?

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The atoms of carbon ¹²₆C, ¹³₆C and ¹⁴₆C can be described as isotopes. Isotopes are atoms of the same element that have different numbers of neutrons in their nuclei. These isotopes of carbon all have six protons (which define them as carbon), but they have different numbers of neutrons. ¹²₆C has 6 neutrons, ¹³₆C has 7 neutrons and ¹⁴₆C has 8 neutrons. Isotopes have identical chemical properties but have different atomic masses due to their different numbers of neutrons.

Which of the following statements about solids is correct?

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The correct statement about solids is that solid particles cannot be easily compressed. This is because the particles in a solid are tightly packed and have fixed positions due to strong intermolecular forces holding them together. Any attempt to compress a solid would require a significant amount of force to overcome these forces and move the particles closer together. In contrast, liquids and gases can be compressed more easily because their particles are not as closely packed and have more room to move around. Therefore, option D is the correct statement.

Chlorine water is used as a bleaching agent because it is

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Chlorine water is used as a bleaching agent because it is an oxidizing agent. Bleaching is a chemical process that involves the breaking down of chromophores, which are responsible for the coloration of substances. Chlorine water is able to oxidize these chromophores and break them down, which results in the removal of the color from the substance being bleached. The oxidizing power of chlorine water comes from the fact that chlorine is a highly electronegative element, which means that it has a strong tendency to attract electrons. This makes it an effective oxidizing agent, as it is able to strip electrons from other substances and cause them to undergo oxidation.

The alkanol obtained from the production of soap is

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The general gas equation \(\frac{PV}{T}\) = K is a combination of

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The general gas equation \(\frac{PV}{T}\) = K is a combination of Boyle's law and Charles' law. Boyle's law states that at constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure. Charles' law states that at constant pressure, the volume of a fixed mass of gas is directly proportional to its temperature. The general gas equation combines these two laws and adds in the ideal gas law constant, K, to relate the pressure, volume, and temperature of a gas. It is important to note that the ideal gas law assumes that the gas behaves ideally, which means that its particles are infinitely small and there are no attractive or repulsive forces between them.

Chemical equilibrium is attained when

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Metals can be stretched into wires because they are

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Metals can be stretched into wires because they are ductile. Ductility is the ability of a metal to be stretched into thin wires without breaking. This property is due to the ability of the metallic bonds between atoms to stretch without breaking. As a result, metals can be drawn into thin wires, making them useful in electrical wiring and other applications.

Consider the following reaction equation
H₃O⁺_(aq) + OH_(aq) \(\rightarrow\) 2H₂O₍₁₎
The reaction represents

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The reaction equation H₃O⁺ + OH^- \(\rightarrow\) 2H₂O represents a neutralization reaction, where a hydrogen ion (H⁺) from an acid (H₃O⁺) reacts with a hydroxide ion (OH^-) from a base to produce water (H₂O) and form a neutral solution. Therefore, the answer is neutralization.

Which of the following arrangements shows increasing order of reactivity of the halogens?

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Amino acids are obtained from proteins by

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Amino acids are the building blocks of proteins. They are linked together by peptide bonds to form a polypeptide chain, which then folds into a three-dimensional protein structure. Proteins can be broken down into their constituent amino acids by hydrolysis, which is the addition of water to break the peptide bonds. Therefore, the correct answer is hydrolysis.

The quality of electricity required to discharge 1 mole of univalent ion is

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The quality of electricity required to discharge 1 mole of univalent ion is 96500C. This quantity of electricity is known as Faraday's constant, which is equivalent to the charge on one mole of electrons (6.022 x 10^23 electrons). When one mole of an univalent ion is discharged, it means that one mole of electrons is transferred, and therefore, the charge required for this transfer is equal to the charge on one mole of electrons, which is 96500C.

The compound that makes palm wine taste sour after exposure to the air for few days is

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On evaporation to dryness, 350³ of saturated solution of salt Z gave 55.5g of salt. What is the solubility of the salt? [Z = 101]

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The solubility of a salt is defined as the maximum amount of solute that can be dissolved in a given amount of solvent at a specified temperature and pressure. Given that 350³ of saturated solution of salt Z gave 55.5g of salt. We can find the solubility of the salt using the formula: Solubility = Mass of solute / Volume of solution First, we need to convert the given mass of salt to moles using its molar mass: Molar mass of Z = 101g/mol Number of moles of Z = 55.5g / 101g/mol = 0.5495 mol Now, we can calculate the volume of the solution using the given volume of 350³: Volume of solution = 350³ = 0.35 dm³ Substituting the values into the formula, we get: Solubility = 0.5495 mol / 0.35 dm³ = 1.57 moldm^-3 Therefore, the solubility of salt Z is 1.57 moldm^-3.

(a) (i) Draw the structures of the isomers of the alkene with molecular formurat C\(_4\)H\(_8\)

(ii) State the class of alkanols to which each of the following compounds belongs:

I. CH\(_3\)C(CH\(_3\))\(_2\)OH;

II. CH\(_3\)CH(CH\(_3\))CH\(_2\)OH;

III. CH\(_3\)CH\(_2\)CH(CH\(_3\))OH.

(b) (i) Write the formulae of the products formed in the following reactions:
I. CH\(_3\)CH\(_2\)COOH \(\frac{K_{(s)}}{}\)

II. CH\(_3\)CH\(_2\)COOH. \(\frac{C_4H_6OH, heat}{Conc.H_2SO_4}\)

III. CH\(_3\)CH\(_2\)CH\(_2\)CH\(_2\)OH \(\frac{H^+/KMnO_4}{(excess)}\)

(ii) Name the major product(s) of each of the reactions in (b)(i).

(c) A gaseous hydrocarbon R of mass 7.0 g occupies a volume of 2.24 dm\(^3\) at s. t.p. If the percentage composition by mass of hydrogen is 14.3, determine its:

(i) empirical formula;

(ii) molecular formula. [ H = 1.00, C = 12.0, Molar volume of gas at s.t.p, = 22.4 dm\(^3\) ]

(d) Define structural isomerism.

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None

TEST OF PRACTICAL KNOWLEDGE QUESTION

All your burette readings (initials and final) as well as the size of your pipette must be recorded but no account of experimental procedure is required. All calculations must be done in your answer booklet

(a) What difference in physical properties enable the separation of mixtures by:

(i) simple distillation,

(ii) paper chromatography;

(iii) fractional distillation.

(b) Give a reason for each of the following practices during titration in the laboratory.

(i) White tile is placed under the conical flask.

(ii) Burette readings are always recorded to two decimal places.

(iii) Calculate the volume of 2.5 moldm\(^{-3}\) stock HČI required to prepare 500 cm\(^3\) of 0.20 moldm HCI. 

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None

TEST OF PRACTICAL KNOWLEDGE QUESTION

All your burette readings (initials and final) as well as the size of your pipette must be recorded but no account of experimental procedure is required. All calculations must be done in your answer booklet 

A solution of 0.050 moldm\(^3\) H\(_2\)C\(_2\)O\(_4\) (ethanedioic acid). B is a solution of KMnO\(_4\), (potassium tetraoxomanganate (VII), of unknown concentration.

(a) Put B into the burette. Pipette 20.0 cm\(^3\) or 25.0 cm\(^3\) of A into a Conical flask and add about 10.0 cm\(^3\) of dilute H\(_2\)SO\(_4\), Heat the mixture to about 40°C - 50°C and titrate it while still hot with B. Repeat the titration to obtain consistent titre values. Tabulate your results and calculate the average volume of B used. The equation of reaction is;

2MnO\(_{4(aq)}^-\) + 5C\(_2\)O\(_{4(aq)}^{2-}\) + 16H\(^+_{(aq)}\) \(\to\)  2MnH\(^{2+}_{(aq)}\) + 8H\(_2\)O\(_{(l)}\) + 10CO\(_{2(g)}\)

(b) From your results and the information provided, calculate the:

(i) concentration of MnO\(_2^-\)  in B in moldm\(^{-1}\) 

(ii) concentration of KMnO\(_4^-\) in B in gdm\(^{-3}\)

(iii) volume of CO\(_2\) evolved at s.t.p when 25.0 cm\(^3\) of H\(_2\)C\(_2\)O\(_4\) reacted completely. [0 = 16.0, K= 39.0, Mn = 55.0, Molar volume of gas at s.t.p.= 22.4 dm\(^3\) mol\(^{-1}\)]

Credit will be given for strict adherence to the instructions. for observations precisely recorded and jor accurate inferences. All tests, observations and inferences must be clearly entered in your answer book in ink, at the time they are made

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(a)(i) Name a suitable drying agent for the preparation of carbon (IV) oxide in the laboratory.

(ii) Using one chemical test, distinguish between carbon (II) oxide and carbon (IV) oxide.

(b)(i) Describe briefly how oxygen and nitrogen could be obtained separately from air on an industrial scale

(ii) State how a lighted splint can be used to distinguish between samples of oxygen and nitrogen.

(c)(i) Give one reason why bauxite is usually preferred as the ore for the extraction of aluminium.

(ii). List two main impurities. usually present in bauxite.

(iii) State the function of sodium hydroxide solution in the extraction of aluminium from its ore.

(iv) Explain briefly why it is difficult to extract aluminium by chemical reduction of aluminium oxide

(v) Write an equation for the reaction of aluminium oxide with aqueous sodium hydroxide.

(d) (i) The melting and boiling points of sodium chloride are 801 °C and 141.3 °C respectively. Explain briefly why sodium chloride does not conduct electricity at 25°C but does so between 801 °C and 1413 °C.

(ii) State the reason why sodium metal is stored under paraffin oil in the laboratory.

(e)(i) State what would be observed when aqueous sodium trioxocarbonate(IV) is added to a solution containing iron (III) ions

(ii) Write a balanced equation for the reaction in (e)(i).

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None

TEST OF PRACTICAL KNOWLEDGE QUESTION

All your burette readings (initials and final) as well as the size of your pipette must be recorded but no account of experimental procedure is required. All calculations must be done in your answer booklet 

C is a mıxture of two salts, containing one cation and two anions. Carry out the following exercises on C. Record your observations and identify any gas(es) evolved. State the conclusion you draw from the result of each test.

(a) Put all of C in a beaker and add about 10 cm\(^3\) of distilled water. Stir well and filter. Keep the filtrate and the residue.

(b) To about 2 cm\(^3\) of the filtrate, add few drops of AgNO\(_{(aq)}\), followed by HNO\(_{3(g)}\). Add excess NH\(_{3(aq)}\) to the resulting mixture.

(c)(i) Put all of the residue into a clean test tube and add about 5 cm of HNO\(_{3(aq)}\)

(ii) To about 2 cm\(^3\) of the solution from 2(c)(i), add NaOH\(_{(aq)}\) in drops and then in excess

(iii) To another 2 cm\(^3\) of the solution from 2(c)(i), add NH\(_{3(aq)}\) in drops and then in excess.

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