WAEC SSCE - Chemistry - 2000
Question 1 Report
Which of the following on burning in air contributes to acid rain?
Answer Details
Sulphur, when burned in air, contributes to the formation of sulphur dioxide gas (SO2). This gas, when released into the atmosphere, can react with water and oxygen to form sulphuric acid (H2SO4), which is a major contributor to acid rain. Therefore, sulphur is the correct answer. The other options, magnesium, aluminium, and zinc do not contribute to acid rain when burned in air.
Question 2 Report
Which of the following is correct about both compounds show below? CH3CH 2CH2OH;CH 3
CH 2CH(OH)CH3
Answer Details
Question 3 Report
An element Z has a combining power of 3. Which of the following formulae is correct of its compounds?
Answer Details
Question 4 Report
Which of the following increases as boiling water changes to steam?
Answer Details
Question 5 Report
A plastic which cannot be softened by heat is described as
Answer Details
A plastic which cannot be softened by heat is described as a "thermosetting" plastic. Thermosetting plastics are a type of polymer that irreversibly hardens or "sets" when heated. They become strong and rigid and cannot be melted or reshaped by heating, unlike thermoplastics which can be melted and reshaped multiple times by heating. Examples of thermosetting plastics include Bakelite and melamine.
Question 6 Report
Which of the following salts is stable to heat?
Question 7 Report
An iron nail placed in a solution copper (ll) tetraoxosulphate (VI) is soon covered with a deposit of copper which of the following equations represents the reactions ?
Answer Details
The correct equation that represents the reaction is: Fe(s) + Cu^2+ (aq) → Fe^2+ (aq) + Cu(s) Explanation: When an iron nail is placed in a solution of copper(II) sulfate, the iron atoms on the surface of the nail lose electrons and become Fe^2+ ions, which go into the solution. At the same time, the Cu^2+ ions from the copper(II) sulfate solution gain electrons from the iron nail and form a solid copper deposit on the surface of the nail. This is a redox reaction, in which iron is oxidized and copper is reduced. The correct equation must show the transfer of electrons from the iron to the copper ions, as well as the formation of solid copper. Only option (D) shows the correct transfer of electrons and formation of a solid copper deposit, making it the correct equation.
Question 8 Report
Chlorine atom forms CI by
Answer Details
Chlorine atom has 7 electrons in its outermost shell, and it needs 1 more electron to complete its octet and become stable. Therefore, it tends to gain 1 electron from another atom to form a stable chloride ion, Cl-. This process is called gaining one electron, and it is represented by the following equation: Cl + e- → Cl- So the correct answer is "Gaining one electron".
Question 9 Report
Which of the following gases is colourless, odourless and soluble in potassium hydroxide solution?
Answer Details
Question 10 Report
What is the value of x in the following equation? Cr2O72- + 14H+ + xe- → 2Cr3+ + 7H2O
Answer Details
Question 11 Report
A finely divided from of a metal burns more readily in air than the rod from because the rod has
Answer Details
A finely divided form of a metal burns more readily in air than the rod form because of its larger surface area. When the surface area of a metal is increased, more of it is exposed to the air, which can lead to increased reactivity. The increased surface area of the finely divided form allows more oxygen molecules to collide with the metal atoms, resulting in a faster and more vigorous reaction. On the other hand, the rod form of a metal has a smaller surface area, making it less reactive as fewer metal atoms are exposed to the air. Therefore, the correct answer is "smaller surface area".
Question 12 Report
A radioactive solid is best stored
Answer Details
A radioactive solid should be stored in a box lined with lead. This is because lead is a dense material that can block radiation, preventing it from escaping and harming people or the environment. Storing the radioactive solid under paraffin oil or in a cool, dark cupboard does not provide sufficient protection from the harmful effects of radiation. Additionally, storing it under ultraviolet light is not recommended as it could potentially increase the radioactive decay of the substance.
Question 13 Report
What type of reaction is involved when wood shavings produce a brown gas with concentrated HNO3?
Answer Details
Question 14 Report
Which of the following contains co-ordinate covalent bond?
Answer Details
The compound that contains a co-ordinate covalent bond is NH4. A co-ordinate covalent bond, also known as a dative bond, is a type of chemical bond where both electrons in the bond originate from the same atom. In NH4, the nitrogen atom donates a pair of electrons to a hydrogen ion, creating an NH4+ ion with a co-ordinate covalent bond. HCI is a polar covalent molecule with a shared pair of electrons. CH4 is a covalent compound where the carbon atom shares electrons with the hydrogen atoms. Na+CI is an ionic compound consisting of a positively charged sodium ion and a negatively charged chloride ion, which are held together by ionic bonds.
Question 15 Report
Which of the following procedures is suitable for identifying the food colouring added to a pastry sample?
Answer Details
To identify the food coloring added to a pastry sample, the suitable procedure is to do a chromatogram of the coloring extract. Chromatography is a technique used to separate and analyze the components of a mixture. The various components will travel at different rates based on their interactions with the stationary phase and mobile phase. In this case, the food coloring extract can be separated into its components and the individual components can be identified based on their characteristic retention times.
Question 16 Report
C8H18 will undergo the following reactions except
Answer Details
C8H18 is a hydrocarbon, which means it consists of hydrogen and carbon atoms only.
(i) Cracking: It is a process of breaking down larger hydrocarbons into smaller hydrocarbons. C8H18 can undergo cracking, which means it can break down into smaller hydrocarbons.
(ii) Combustion: It is a reaction between a substance and oxygen in the presence of a flame or spark. C8H18 can undergo combustion and produce carbon dioxide and water.
(iii) Substitution: It is a reaction in which an atom or group of atoms is replaced by another atom or group of atoms. C8H18 can undergo substitution if it reacts with a suitable reagent.
(iv) Addition: It is a reaction in which two or more reactants combine to form a larger product. C8H18 can undergo addition if it reacts with a suitable reagent.
Therefore, C8H18 can undergo all of the above reactions. So, the answer is None.
Question 17 Report
The atoms of four elements are represented as 20Q, 16R, 10S and 8T Which of the elements would be unreactive?
Answer Details
Question 18 Report
What is the mass number of an element if its atom contains 10 protons, 10 electrons and 12 neutrons?
Answer Details
The mass number of an element is the sum of the number of protons and neutrons in the nucleus of an atom. Given that the atom of the element has 10 protons and 12 neutrons, the mass number of the element would be: Mass number = Number of protons + Number of neutrons Mass number = 10 + 12 Mass number = 22 Therefore, the answer is: 22.
Question 19 Report
Which of the following salts is stable to heat?
Answer Details
Silver nitrate (AgNO3) is the salt that is stable to heat. Stability to heat refers to a salt's ability to resist decomposition or breakdown when exposed to high temperatures. Silver nitrate is a relatively stable salt that does not decompose easily even when exposed to high heat. This property makes it useful in various industrial and laboratory applications that involve heating, such as in the production of photographic film. In contrast, potassium carbonate (K 2CO 3), ammonium sulfate ((NH 4) 2SO 4), and sodium bicarbonate (NaHCO3) are not as stable to heat and may decompose or break down when exposed to high temperatures.
Question 20 Report
An element Z has a combining power of 3. Which of the following formulae is correct of its compounds?
Answer Details
The correct formula for the compound of element Z would be Z2O3. This is because Z has a combining power of 3, meaning that it can form compounds by bonding with three other elements. In Z2O3, each Z atom is bonded to three O atoms, satisfying Z's combining power of 3. None of the other options satisfy this requirement, as they either have too few or too many atoms of Z.
Question 21 Report
Given that the electronic configuration of an element X is 1s22s22p63s 23p4, it can be deduced that X
Answer Details
The electronic configuration of an element X is given as 1s22s22p63s 23p4. This indicates that the element X has a total of 16 electrons. In the electronic configuration, the last electron enters the 3p subshell. Since there are 4 electrons present in the 3p subshell, this means that the element X belongs to the 6th group of the periodic table (also known as group VI), which contains elements with 6 valence electrons. Therefore, the correct option is "belongs to group VI in the Periodic Table". The other options are incorrect as there is no information in the given electronic configuration to support those statements.
Question 22 Report
9.60 g of a gas X occupies the same volume at 0.30 g of hydrogen under the same conditions. Calculate the molar mass of X [H = 1]
Answer Details
The molar volume of gases at standard temperature and pressure (STP) is the same for all gases. This means that equal volumes of gases at STP contain equal numbers of molecules. The molar volume of a gas at STP is 22.4 L/mol. From the question, we know that: mass of gas X = 9.60 g mass of hydrogen = 0.30 g We can use the molar masses of hydrogen and gas X to calculate the number of moles of each gas: moles of hydrogen = mass/molar mass = 0.30 g/1 g/mol = 0.30 mol moles of gas X = mass/molar mass = 9.60 g/molar mass Since the two gases occupy the same volume, we can equate their molar volumes: moles of hydrogen/volume = moles of gas X/volume Substituting the values we know: 0.30/22.4 = (9.60/molar mass)/22.4 Solving for the molar mass of gas X: molar mass = (9.60/0.30) x 1 = 32 g/mol Therefore, the molar mass of gas X is 32 g/mol. Answer: 32g mol -1
Question 23 Report
Electrovalent compounds are characterized by
Answer Details
Electrovalent compounds, also known as ionic compounds, are characterized by a high melting point. This is because they have a lattice structure made up of positive and negative ions that are held together by strong electrostatic forces of attraction. These forces require a lot of energy to break, hence the high melting point of electrovalent compounds. Additionally, electrovalent compounds tend to be brittle, have high boiling points, and are good conductors of electricity in their molten or aqueous states due to the presence of charged ions. Solubility in ethanol or strong oxidizing ability are not defining characteristics of electrovalent compounds.
Question 24 Report
What is the effect of using vanadium (V) oxide as catalyst in the reaction represented by the following equation? 2SO2 + O2 ⇌ 2SO3; ∆H = - xKJmol-1
Answer Details
Question 25 Report
Which of the following occurs when a solution of CuSO4 is electrolysed using copper electrodes?
Answer Details
When a solution of CuSO4 is electrolyzed using copper electrodes, the cathode becomes coated with copper. This happens because during electrolysis, positively charged copper ions (Cu2+) migrate towards the negatively charged cathode, where they receive electrons from the electrode and are reduced to neutral copper atoms. These copper atoms then combine and deposit on the surface of the cathode, causing it to become coated with copper. The other options are incorrect because: - Both electrodes do not gain electrons; rather, the cathode gains electrons while the anode loses electrons. - The blue color of the solution fading gradually is not a specific outcome of the electrolysis of CuSO4. - The anode does not increase in mass; rather, it loses mass due to the oxidation reaction that occurs at the anode during electrolysis.
Question 26 Report
Which of the following non-metals reacts most readily with metals?
Answer Details
Out of the given options, chlorine reacts most readily with metals. Chlorine is a highly reactive non-metal that readily reacts with most of the metals to form ionic compounds called metal chlorides. When chlorine gas comes into contact with a metal, it gains one electron to form chloride ions, which have a stable electronic configuration of a noble gas. The reaction is exothermic and produces a white solid or colorless gas, depending on the metal. Chlorine gas is used in many industries, such as water treatment, chemical manufacturing, and paper production, due to its strong oxidizing properties and ability to react with metals. Therefore, the correct answer is "Chlorine".
Question 27 Report
A colourless, odourless liquid T, gives effervesce with sodium trioxocarbonate (IV) and a white precipitate with silver trioxonitrate (V) solution T is mose probably
Question 28 Report
0.10 mol dm-3 NaCI conducts electricity better than 0.10 mol dm-3 CH3COOH because the solution of NaCI
Answer Details
0.10 mol dm-3 NaCI conducts electricity better than 0.10 mol dm-3 CH3COOH because the solution of NaCI contains more ions. When an ionic compound like NaCI dissolves in water, it dissociates into its component ions, Na+ and Cl-. These ions are able to carry an electric charge and are therefore able to conduct electricity. In contrast, CH3COOH is a weak acid that only partially dissociates in water to form CH3COO- and H+ ions. Since there are fewer ions in the solution of CH3COOH compared to NaCI, it conducts electricity less efficiently. Therefore, the correct answer to the question is that the solution of NaCI contains more ions.
Question 29 Report
Which of the following needs to be hydrolysed before it shows reducing property?
Answer Details
Sucrose needs to be hydrolysed before it shows reducing property. Sucrose is a non-reducing sugar, meaning it does not have a free aldehyde or ketone group that can participate in oxidation-reduction reactions. To show reducing property, it needs to be hydrolyzed into its component monosaccharides, glucose, and fructose. This is because glucose and fructose are reducing sugars as they have free aldehyde and ketone groups that can participate in oxidation-reduction reactions. Thus, hydrolysis of sucrose is necessary to break the glycosidic bond between glucose and fructose and convert them to free sugars that can show reducing properties.
Question 30 Report
The gas evolved when dilute tetraoxosulphate (VI) acid reacts with sodium hydrogen trioxocarbonate (IV) is
Answer Details
The reaction between dilute tetraoxosulphate (VI) acid (H2SO4) and sodium hydrogen trioxocarbonate (IV) (NaHCO3) produces carbon (IV) oxide (CO2) gas. This can be explained by the reaction equation: H2SO4 + 2NaHCO3 → Na2SO4 + 2CO2 + 2H2O As can be seen from the equation, carbon (IV) oxide gas is produced as one of the products. Therefore, the gas evolved when dilute tetraoxosulphate (VI) acid reacts with sodium hydrogen trioxocarbonate (IV) is carbon (IV) oxide gas.
Question 31 Report
Which of the following compounds dissolves in water to give an alkaline solution?
Answer Details
Among the given options, only potassium oxide dissolves in water to give an alkaline solution. When potassium oxide (K2O) is dissolved in water, it reacts with water to form potassium hydroxide (KOH), which is a strong base. The chemical equation for this reaction is: K2O + H2O → 2KOH Hence, the solution formed is alkaline due to the presence of hydroxide ions (OH-) from the dissociation of the potassium hydroxide. The other compounds listed do not produce hydroxide ions when dissolved in water, and therefore do not give an alkaline solution.
Question 32 Report
Which of the following will displace copper from a solution of copper (ll) salt?
Answer Details
Question 33 Report
Elactrostatic force of attraction between sodium ion and halide ion is greatest in
Answer Details
Question 34 Report
What is the shape of a molecule of CCI4?
Answer Details
The shape of a molecule is determined by its electron pair geometry, which is based on the number of electron groups around the central atom. In the case of CCl4, there are four bonding pairs of electrons and no lone pairs around the central carbon atom. This gives it a tetrahedral electron pair geometry, which corresponds to a tetrahedral molecular shape. Therefore, the correct answer is "Tetrahedral".
Question 35 Report
P,Q,R and S are metals in the same group in the Periodic Table but in periods 3,4, 5 and 6 respectively which of them loses electrons least readily?
Answer Details
The elements in the same group of the periodic table have the same number of valence electrons. Valence electrons are the electrons located in the outermost shell of an atom that are involved in chemical bonding. The valence electrons determine the reactivity and chemical properties of an element. In this case, all four metals are in the same group and have the same number of valence electrons. However, as we move from left to right across a period, the atomic radius decreases and the effective nuclear charge (the attractive force experienced by the valence electrons from the nucleus) increases. This makes it harder for the valence electrons to be removed from the atom, so the ionization energy (the energy required to remove an electron) increases. Therefore, S, which is in period 6 and has the highest effective nuclear charge, loses electrons least readily. The correct answer is S.
Question 36 Report
Chemical equilibrium is attained when
Answer Details
Chemical equilibrium is attained when the concentrations of the reactants and products remain constant, and the forward and reverse reactions are occurring at the same rate. In other words, the concentrations of the reactants and products do not change over time. This does not mean that the reactants have stopped forming products; it simply means that the rate of the forward reaction is equal to the rate of the reverse reaction. At equilibrium, the system is balanced, and the reaction is said to be in a steady state.
Question 37 Report
Allotropes of an element differ in their
Answer Details
Allotropes of an element are different forms or structures of the same element in the same physical state. They differ in their physical properties, such as color, melting point, boiling point, and density, due to the variations in the arrangement of atoms or molecules. For example, diamond and graphite are allotropes of carbon, and they have different physical properties because of their different atomic arrangements. Although allotropes have different physical properties, they have the same chemical properties, as they are composed of the same element with the same number of protons and electrons. Therefore, the correct answer is "physical properties".
Question 38 Report
In which of the following is the oxidation number of sulphur equal to -2?
Answer Details
S8, H2S, SO2, and SO32- are all compounds that contain sulfur, but the oxidation number of sulfur is only -2 in one of them. The oxidation number of an atom is a measure of the number of electrons that it has gained or lost in a chemical reaction. In S8, the oxidation number of sulfur is zero because it is in its elemental state and has not gained or lost any electrons. In H2S, the oxidation number of sulfur is -2 because hydrogen has an oxidation number of +1 and the overall charge of the compound is 0. In SO2, the oxidation number of sulfur is +4 because oxygen has an oxidation number of -2 and the overall charge of the compound is 0. In SO32-, the oxidation number of sulfur is +4 because oxygen has an oxidation number of -2 and the overall charge of the ion is -2. Therefore, the only compound in which the oxidation number of sulfur is -2 is H2S.
Question 39 Report
Two-organic substances are labelled K and L if K gave a blue-black colour with iodine solution and L gave a deep red precipitate with Million's reagent, it can be concluded that
Answer Details
From the given information, it can be concluded that K is a carbohydrate and L is a protein. This is because the blue-black colour with iodine solution is a characteristic test for the presence of starch, which is a type of carbohydrate. On the other hand, the deep red precipitate with Million's reagent is a characteristic test for the presence of proteins. Therefore, based on the tests carried out, K is a carbohydrate and L is a protein.
Question 41 Report
Biotechnology is applied in the following except
Answer Details
Biotechnology is applied in the production of various useful products using biological organisms or their components. Baking industry and wine production both use biotechnology in their processes. Production of antibiotics involves the use of biotechnology to produce these drugs using microorganisms like bacteria and fungi. However, the manufacture of soap does not involve the use of biotechnology. Soap is typically made from natural or synthetic ingredients using chemical reactions rather than biological processes. Therefore, the answer is "manufacture of soap."
Question 42 Report
Which of the following procedures is suitable for identifying the food colouring added to a pastry sample?
Answer Details
The suitable procedure for identifying the food coloring added to a pastry sample is to do a chromatogram of the coloring extract. Chromatography is a technique that separates and identifies the components of a mixture. In this case, a small amount of the coloring extract can be applied to a special paper, and then a solvent is used to separate the components of the extract. The different components will travel at different speeds, allowing for the identification of the specific food coloring used in the pastry sample. This method is more specific and reliable compared to the other options provided, such as carrying out some food tests or examining the pastry sample under a microscope, which may not provide conclusive results. Determining the molar mass of the coloring is also not a suitable method for identifying the food coloring added to the pastry sample.
Question 43 Report
If 20 cm3 of distilled water is added to 80 cm3 of 0.50 mol dm-3 hydrochloric acid, the concentration of the acid will change to
Answer Details
When 20 cm3 of distilled water is added to 80 cm3 of 0.50 mol dm-3 hydrochloric acid, the total volume of the solution becomes 100 cm3. However, the amount of HCl molecules in the solution remains the same before and after the dilution. Therefore, we can use the formula: C1V1 = C2V2 where C1 and V1 are the initial concentration and volume of the acid, and C2 and V2 are the final concentration and volume of the acid after dilution. Substituting the values, we get: C1V1 = C2V2 (0.50 mol dm-3) x (80 cm3) = C2 x (100 cm3) C2 = (0.50 mol dm-3) x (80 cm3) / (100 cm3) C2 = 0.40 mol dm-3 Therefore, the concentration of the acid will change to 0.40 mol dm-3 after the dilution. Thus, the correct option is (B) 0.40 mol dm-3.
Question 44 Report
The type of chemical bond that exists between potassium and oxygen in potassium oxide is
Answer Details
The chemical bond that exists between potassium and oxygen in potassium oxide is ionic. In an ionic bond, electrons are transferred from one atom to another resulting in the formation of positively charged cations and negatively charged anions. In potassium oxide, potassium (K) loses one electron to form a K+ cation, while oxygen (O) gains two electrons to form an O2- anion. The resulting electrostatic attraction between the oppositely charged ions leads to the formation of an ionic bond. Therefore, the bond between potassium and oxygen in potassium oxide is ionic because electrons are transferred from potassium to oxygen to form K+ and O2- ions.
Question 45 Report
When sodium hydroxide solution is added to a solution of zinc salt, the white precipitate fromed redissolves in excess sodium hydroxide because
Answer Details
Question 46 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
All your burette readings (initial and final), as well as the size of your pipette, must be recorded but on no account of experimental procedure is required. All calculations must be done in your answer book.
A is solution of trioxonitrate (V) acid, B is a solution containing 6.90 g of potassium trioxocarbonate (IV) per dm\(^3\)
(a) Put A into the buret and titrate it against 20.0 cm\(^3\) or 25.0 cm\(^3\) portions of B using methy orange or screened methyl orange as indicater. Record the volume of your pipette. Tabulate your burette readings and calculate the average volume A used. The equation for the reaction is K\(_2\)CO\(_{3(aq)}\) + 2HNO\(_{3(aq)}\) \(\to\) 2KNO\(_{3(aq)}\) + CO\(_{2(g)}\) + H\(_2\)O\(_{(l)}\)
(b) From your results and the information provided calculate;
(i) concenytration of solution B in mol dm\(^{-3}\)
(ii) number of potassium ions in 1.00 dm\(^3\) of B [C = 12.0, O = 16.0, K = 39.0, Avogadro constant = 6.02 x 10\(^{23}\) mol \(^{-1}\)]
Question 47 Report
(a) What is meant by each of the following terms?:
(i) Esterification
(ii) Saponification
(b)(i) Give the general moluecular 1 formula of alkynes
(ii) Write the molecular formula and empirical formula of ethylethanoate.
(iii) Draw the structure of 1, 1, 2, 2-tetrabromoethane
(iv) Write an equation for the reaction of ethanol with sodium
(c) Consider the following reaction schemes:
I II
Petroleum ---> Petroleum Fractions. Higher Petroleum Fractions ---> Petrol + X
(i) State type of process/reaction involved in each of the stages labelled I to IV.
(ii) Identify X and Y
(iii) Give the IUPAC name of the product obtained in stage III.
(iv) What are the reaction conditions for stage IV?
(d) Explain why palm wine: (i) froths or foams (ii) tastes sour after some days.
Answer Details
None
Question 48 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
Credit will be given for strict adherence to instructions, for observations precisely recorded and for accurate inferences. All tests observations and inferences must be clearly entered in your answer book. in ink, at the time they are made.
C is a mixture of two simple salts. Carry out the following exercises on C. Record your observations and identify any gases evolved. Sate the conclusion you draw from the result of each test.
(a) Put all of C into a beaker of boiling tube and add about 10cm\(^3\) of distilled water. Stir well and filter. Keep the residue and keep the residue and the filtrate. Test the filtrate with litmus
(b) Add about 1 cm\(^3\) of dilute hydrochloric acid to the residue in a test tube and warm gently Divide the reaction mixture into two portions
(c)(i) To the first portion from (b) add saturated sodiuim trioxocarbonate (V) solution in excess
(d) To bout 2cm\(^2\) of the filtrate from (a) add a few drops of barium chloride solution followed by excess dilute hydrochloric acid
Answer Details
None
Question 49 Report
(a)(i) Give the names of two allotropes of sulphur.
(ii) State and explain what is observed when hydrogen sulphide is bubbled through acidified potassium tetraoxomanganatc (VII) solution
(iii) List one product of the reaction of sulphur (IV) oxide with hydrogen sulphide
(b)(i) What are the raw materials for the manufacture of tetraoxosulphate (VI) acid by the contact process?
(ii) Write an equation for the reaction that requires a catalyst in the contact process and state the catalyst used.
(iii) State the observation and the product formed when concentrated H\(_2\)SO\(_4\) reacts with each of the following:
I. Copper turnings Ii. A cube of sugar
(c)(i) Give three uses of sodium trioxocarbonate (IV).
(ii) What name is given to reactions of the following type?:
exposure to air
Na\(_2\)CO\(_3\) + 10H\(_2\)O\(_{(s)}\) \(\to\) Na\(_2\)CO\(_3\); H\(_2\)O\(_{(S)}\) + 9H\(_2\)O
(iii) Calculate the solubility of Na\(_2\)CO\(_3\) at 25°C, if 2.0 cm\(^3\) of its saturated solution at that temperature gave 1.75g of the anhydrous alt. [C = 12, O = 16, Na = 23].
Question 50 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
(a) Name one laboratory equipment used for
(i) keeping salts dry:
(ii) converting vapour to liquid during distillation
(ii) bubbling a gas into a liquid
(b) (i) What technique would you use to purity a sample of sodium chloride contaminated with ammonium chloride?
(i) Given sodium hydroxide solution, outline tne procedure you would use to determine whether or not all the ammonium chloride in (b)(i) above had been removed
(c) State what is observed on carrying out each of the following exercises.
(i) Adding few drops of methyl orange indicator to lime juice:
(ii) Adding few drops of concentrated HNO\(_3\) to acidified FeSO\(_4\) solution
(iii) Exposing a fresh precipitate of silver chloride to sunlight for 30 minutes
(iv) Adding zinc dust to dilute CuCl\(_2\) solution;
(v) Adding dilute H\(_2\)SO\(_4\), to Pb(NO\(_3\))\(_2\) solution
Answer Details
None
Question 51 Report
a)(i) State Graham's law of diffusion.
(ii) Calculate the vapour density of a triatomic gas X if its relative: atomic mass is 16.
(iii) Equal volumes of gases Y and Z are maintained at the same temperature and pressure. If the mass of a molecule of Y is twice that of Z state and explain which of the molecules has the, greater average velocity.
(b) The graph below is the ratio curve for the following reaction carried out in an open vessel.
MgCO\(_{3(s)}\) + 2HCI\(_{(aq)}\) \(\to\) MgCl\(_{2(aq)}\) + CO\(_{2(g)}\) + H\(_2\)\(_{(l)}\).
(i) For how long did reaction occur?
(ii) Why was there a loss in mass?
(iii) State whether reaction rate was fastest at the beginning, the middle or towards the end of the reaction. Give reason for our answer.
(iv) List three reaction conditions that can affect the slope of the curve
(c) Consider the following reaction at equilibrium: PCI\(_{5(g)}\) \(\rightleftharpoons\) PCI\(_{3(g)}\)); \(\Delta\)H = +95 kJmol\(^{-}\)
(i) Write an expression for the equilibrium constant K.
(ii) Predict the effect of the following on the equilibrium position.
I. Increased pressure
II. Increased temperature
III. Removal of chlorine Sketch an energy profile diagram for the forward reaction.
Answer Details
None
