Document
1. The hydrolysis of proteins by dilute mineraks acids produces
A. sucrose
B. glucose
C. amino acids
D. fatty acids
2. Which of the following oxides causes acid rain?
A. $CO$
B. $NO$
C. $H_2O_2$
D. $NO_2$
3. The ratio of carbon atoms to hydrogen atoms in a hydrocarbon is 1:2. If its molecular mass is 56, what is its molecular formula?
A. $C_3H_6$
B. $C_4H_8$
C. $C_2H_4$
D. $CH_2$
4. See pages for figures
5. Cathodic protection of metals is based on
A. standard electrode potential of hydrogen
B. its electrical conductivity
C. nature of oxides formed
D. relative tendencies of oxidation
6. If humid air is polluted by chlorine discharge, the air can be restored by sprinkling
A. solid $MnO_2$
B. acidified $KMnO_4$
C. acidified $FeSO_{4}$
D. saturated $NaCl_{(aq)}$
7. See pages for figures
8. Which of the following pairs of compounds would form a precipitate when their aqueous solutions are mixed?
A. NaCl and $KNO_3$
B. KCl and $NaNO_3$
C. $K_2SO_4$ and $BaCl_2$
D. $NH_4NO_3$ and $Na_2CO_3$
Q9-11 see pages for figures
12. The formation of ethyene from dehydration of ethanol can be described as
A. an addition reaction.
B. an elimination reaction.
C. an oxidation reaction.
D. a substitution reaction.
13. Which of the following gas is highly soluble in water at room temperature?
A. Ammonia
B. carbon(IV) oxide
C. Chlorine
D. Hydrogen
14. A molecule of a phosphorus is
A. diatomic
B. triatomic
C. tatraatomic
D. monoatomic
15. The most common method of preparing insoluble salts is by
A. filtration
B. decomposition
C. neutralization
D. double decomposition
16. The number of moles of oxygen would exert a pressure of 10 atm at 320K in an 8.2 $dm^{3}$ cylinder? [R = $0.082 atm dm^{3} mol^{-1} K^{-1}$]
A. $0.32$
B. $1.56$
C. $3.13$
D. $31.25$
17. The basic properties of salt is
A. efflorescence
B. high melting point
C. hygroscopy
D. low solubility
18. What would be observed when aqueous Ammonia is added in drops and then in excess to a solution of copper(II) ions?
A. A blue precipitate is formed which is soluble in excess ammonia
B. brick red precipitate is produced which is insoluble in excess ammonia
C. white precipitate is formed which is soluble in excess ammonia
D. green precipitate is formed which is insoluble in excess ammonia
19. When $CuSO_{3(aq)}$ is added to ${P_b}(NO_3)_{2(aq)}$.
A. there would be no visible change
B. a blue precipitate would be formed
C. the resulting solution would be colorless
D. a white precipitate would be formed
20. See pages for figures
21. Under which condition of pressure (P) and temperature (T) would the volume of an inflated ballon increase?
A. both T and P are increased
B. both T and P are decreased
C. T is increased and P is decreased
D. T is decreased and P is increased
22. The collision between ideal gas molecules are considered to be perfectly elastic because
A. they collide without losing energy
B. they move randomly in straight line
C. their average kinetic energy is variable
D. the distance between them is large compared to their sizes
23. Elements with high ionization energy would
A. lose electrons easily.
B. have large atomic radii.
C. have high effective nuclear charges.
D. have low atomic number.
24. Which of the followwing statements about Group VII elements is correct?
A. they are present in the same physical state.
B. they are strong reducing agents.
C. their reactivity decreases down the group
D. they exist as monoatomic molecules
Q25-26 See pages for figures
27. The reactivity of fluorine is high because
A. its high electronegativity
B. the small size of the fluorine atoms
C. the availability of d-orbitals
D. the strong F-F bond
28. How many coulombs of electricity would liberate $1.08_g$ of Ag from a solution of silver salt? [Ag = 108.0; 1 F = 96500C]
A. $96500C$
B. $9650C$
C. $965C$
D. $9.65C$
29. The bohr model of the atom proposed the existence of
A. the nucleus
B. electron shells
C. nucleons
D. neutrons
30. At $25^0C$ evaporation of a $100cm^3$ solutions of $K_2CO_3$ to dryness gave 14g of the salt. What is the solubility of $K_2CO_3$ at $25^0C$? [$K_2CO_3$ = 138]
A. $0.01mol dm^{-3}$
B. $0.101 mol dm^{-3}$
C. $1.01 moldm^{-3}$
D. $10.0 mol dm^{-3}$
31. Student X titrated $25cm^3$ of $Na_2CO_3$ with $0.1 moldm^{}-3$ HCl, using methyl orange as indicator. Student Y carried out the same exercise but used phenolphthalein as indicator. Which of the following statements about the titration is true?
A. Hydrogen chloride gas was released in the reactions in both titrations
B. The titre values obtained from the titrations are equal
C. The titre value obtained by X is twice that of Y
D. The titre value obtained by Y is twice that of X
32. What is the concentration of a solution which contains 0.28g of potassium hydroxide in $100cm^{-3}$ of solution? [KOH = 56]
A. $0.01 {moldm}^{-3}$
B. $0.05 {moldm}^{-3}$
C. $0.10 {moldm}^{-3}$
D. $0.50 {moldm}^{-3}$
33. What is the empirical formula of a hydrocarbon containing $0.160 moles$ of carbon and $0.640$ moles of hydrogen?
A. $CH_2$
B. $CH_3$
C. $CH_4$
D. $C_2H_4$
34. Which of the following species has the largest ionic radius?
A. $S^{2-}$
B. $Cl^-$
C. $K^+$
D. $Ca^{2+}$
35. Which of the following statements are correct about ionization energy?
A. decreases across the periods.
B. results in the formation of an anion.
C. causes metallic nuclei to disintegrate
D. decreases down the group
36. Potassium trioxonitrate(V) can be obtained from its solution by
A. distillation
B. evaporation
C. crystallization
D. filtration
37. An element, $Q$, contains 69% of $^{63}Q$ and 31% of $^{65}Q$. What is the relative atomic mass of Q?
A. $63.0$
B. $63.6$
C. $65.0$
D. $69.0$
38. The following ions have the same electron configuration except $_8O$, $_{12}Mg$, $_{13}Al$, $_{17}Cl$.
A. $Cl^-$
B. $O^{2-}$
C. $Mg^{2+}$
D. $Al^{3+}$
39. The region around the nucleus where electrons can be located is called
A. a spectra
B. an orbital
C. a quanta
D. a field
40. Protons and electrons are called fundamental particles because they
A. are invisible.
B. have different charges.
C. are the lightest particles.
D. are found in all matter.
Q41-Q44 See pages for figures
45.The isotpes of neon are represented by the symbols $^{20}_xNe$, $^{21}_yNe$, $^{22}_zNe$. the relationship between x,y and z is
A. $x>y>z$
B. $x< y< z $
C. $x=y=z$
D. $x< z < y $
46. Which of the following pairs of molecules form hydrogen bonds?
A. $C_2H_5OH$ and $CH_3OH$
B. $CH_3OH$ and $H_2$
C. $H_2S$ and $CH_4$
D. $NH_3$ and $SO_2$
47. Which of the following staements about elements in group VII is correct?
A. $Br_2$ will oxidize $Cl^-$
B. $F_2 $ has the least tendency to be reduced
C. $Cl_2 $ will oxidize $I^-$
D. $I_2$ is a stronger oxidizing agent than $F_2$
48. Electrovalent compounds normally
A. have low boiling point.
B. have mobile electron.
C. conduct electricity in the solid state.
D. dissolve in polar solvents.
49. A coordinate covalent bond could be formed between
A. $NH_3$ and $PCl_3$
B. $BCl_3$ and $AlCl_3$
C. $BCl_3$ and $NH_3$
D. $H+$ and $AlCl_3$
50. Which of the following scientist discovered the electron?
A. Joseph J. Thompson
B. James Chadwick
C. Amedeo Avogadro
D. Ernest Rutherford
WASSCE 2022
1. The by-product of fermentation of sugar is
A. carbon(IV)oxide
B. ethanoic acid
C. propanol
D. propan-$1,2,3$-triol
2. Which of the following sugars is a product of the condensation monosaccharides?
A. Galactose
B. Maltose
C. Glucose
D. Fructose
3. The cleansing effect of soap is low in acidic water because of
A. the formation of unionized fatty acid.
B. increase in the pH of the soap molecules.
C. anti-biodegradable effect on hydrogen ions.
D. the hardness of the acidic water.
4. The following compounds are condensation polymers except
A. nylon
B. protein
C. starch
D. polythene
5. What amount of electricity is required to deposit one mole of aluminium from a solution of $AlCl_3$?
A. One Faraday
B. One ampere
C. Three Faradays
D. Three amperes
6. Which of the following compounds would react rapidly with bromine?
A. Benzene
B. Hexane
C. Hexene
D. hexanol
7.Alkanols can be manufactured from alkenes by the initial reaction of alkenes with
A. bromine in tetrachloromethane
B. concentrated tetraoxosulphate(VI) acid
C. aqueous potassium tetraoxomanganate (VII)
D. sodium hydroxide solution.
8. Which of the following statement about the standard hydrogen electrode is not correct?
A. The hydrogen gas is at a temperature of 1 atmosphere.
B. A solution cantaining $1 moldm^{-3}$ of $H^+_{(aq)}$ ions is used.
C. A platinum electrode is used.
D. The temperature is kept at $20^0C$.
9. If 60g of M combines with 24g of oxygen, what would the empirical foemula of the oxide be? [O = 16.0, M = 120]
A. $MO$
B. $MO_2$
C. $MO_3$
D. $MO_4$
10. The product of the electrolysis of dilute sodium chloride using carbon electrode are
Anode Cathode
A. chlorine and sodium
B. oxygen and hydrogen
C. chlorine and hydrogen
D. hydrogen and oxgen
11. Determine the quantity of electricity used when a current of 0.20 amperes is passed through an electrolytic cell for 60 minutes.
A. $12C$
B. $120C$
C. $360C$
D. $720C$
12. Oxochlorated(I) acid is used as a bleaching agent because it is
A. a weak acid
B. a reducing agent
C. an oxidising agent
D. a strong acid
13. The IUPAC name for $CH_3CHCH_3CHClCH_3CH_2CH_3$ is.
A. 2,4-dimethyl-3-chlorohexane
B. 3,5-dimethyl-4-chlorohexane
C. 4-chloro-3,5-dimethylhexane
D. 3-chloro-2,4-dimethylhexane
14. A colorless gas with pungent smell is evolved when when dilute hydrochloric acid is added to a sample of salt. The gas evolved could turn
A. acidified $K_2Cr_2O_7$ solution colourless.
B. acidified $KMnO_4$ solution colorless.
C. $Fe(NO_3)_2$ solution green.
D. $Pb(NO_3)_2$ paper black.
15. If 5.0g of marble reacts with 25.0$cm^3$ hydrochloric acid, which of the following combinations has the fastest reaction rate?
A.Marble chips and $2.0 moldm^3$ HCl $_{(aq)}$
B. Marble chips and $2.5 moldm^3$ HCl $_{(aq)}$
C. Powdered marble and 2.5 $moldm^3$ HCl ${(aq)}$
D. Powdered marble and $2.0 moldm^3$ HCl${(aq)}$
16. Increasing the temperature generally
A. decrease the solubility of a solid in a liquid but increases the solubility of a gas in a liquid.
B. increases the solubility of a solid in a liquid but decreases the solubility of a gas in a liquid.
C. increases the solubility of both a solid and a gas in a liquid.
D. decreases the solubility of both a solid and a gas in a liquid.
17. A white precipitate was formed when $BaCl_{2(aq)}$ was added to an aqueous solution of a salt X. The precipitatedissolved in dilute HCl with rapid effervescence. salt X is likely to contain.
A. $SO_4^{2-}$ ions
B. $ZO _3^{2-}$ ions
C. $NO_3^-$ ions
D. $CO_3^{2-} ions$
18. Before a reaction could take place, there should be
A. ionisation of reactant particles.
B. breakage of bonds of products.
C. breakage of bonds of reactants.
D. ionisation of product particles.
19. Consider the following reaction equation: CaO $SiO_2$ $\longrightarrow$ $CaSiO_3$
Silicon(IV)oxide is acting as
A. a basic oxide
B. a reducing agent
C. an acidic agent
D. an oxidising agent
20. Which of the following acids would form normal salt only?
A. Tetraoxosulphate(VI) acid
B. Trioxonitrate(V) acid
C. Tetraoxosulphate(V) acid
D. Trioxosulphate(IV) acid
21. What is the partial pressure of oxygen at s.t.p in gaseous mixture containing $100cm^3$ of oxygen and $900cm^3$ of nitrogen gas?
A. $1.0atm$
B. $0.1atm$
C. $9.0atm$
D. $0.9atm$
22. Graphite is used as a dry lubricant due to the presence of
A. mobile electrons
B. free electrons
C. octahedral structures
D. layered structures
23. Which of the following gases is alkaline?
A. $NO_2$
B. $CO_2$
C. $NH_3$
D. $N_2O$
24. Which of the following statements about an equilibrum system is correct?
A. Forward and backward reactions occur at the same rate.
B. The concentration of reactants and products can be changed by adding a catalyst.
C. The concentration of reactants and products are not affected by a change in temperature.
D. Forward and backward reactions occur at different rate
25. See pages for figures
26. When air in syringe is compressed such that there is no change in temperature, the
A. air liquifies
B. pressure increases
C. intermolecular space increases
D. density increases
27. Which of the following statements about liquid is/are true? I. Liquids mantain their volume at constant temoperature II. Liquids have fixed shape III. Liquids do not diffuse IV. Change in pressure affects volume of liquids
A. I only
B. IV only
C. I and IV only
D. II and III only
28. Hydrogen chloride gas reacted with oxygen gas to yield water and chlorine gas. The mole ratio of the hydrogen chloride gas to water is
A. $1:3$
B. $2:1$
C. $3:1$
D. $4:1$
29. What number of moles of oxygen would exert a pressure of $10atm$ at $320$ K in an $8.2$ dm^3 cylinder? [R = 0.082 $atm dm^{-3}mol^{-1}k^{-1}$]
A. $0.32$
B. $1.52$
C. $3.13$
D. $31.25$
30. If 50cm3 of a saturated solution of $KMnO_3$ at $40^0C$ contained 5.05g of the salt, its solubility at the same temperature would be [$KNO_3$ = 101]
A. $1.0moldm^{-3}$
B. $1.5moldm^{-3}$
C. $2.0moldm^{-3}$
D. $5.0moldm^{-3}$
31. Which of the following elements would displace copper from a solution of copper ions?
A. Silver
B. Gold
C. Lead
D. Mercury
32. What is the percentage composition of carbon in $Ca(HCO_3)_2$? [Ca = 40, O = 16.0, C = 12.0, H = 1.0]
A. 22.2%
B. 14.8%
C. 7.4%
D. 3.7%
33. Which of the following types is intermolecular?
A. Covalent bond
B. Hydrogen bond
C. Ionic bond
D. Metallic bond
34. The maximum number of covalent bonds formed by nitrogen is
A. 1.
B. 2.
C. 3.
D. 4.
35. The IUPAC name of thhe compound $C{H_3}CH(C{H_3})CHC{H_2}$
A. 2-methyl- but-1-ene
B. 2-methyl but-2-ene
C. 3-methyl but-1-ene
D. 3-methyl but-2-ene
36. Ionisation energy increases across the period in the periodic table because
A. atomic number increases.
B. effective nuclear charge increases.
C. mass number decreases
D. screening sffect decreases
37. Which of the following propeeties indicate that an element is a metal. I. reacts with oxygen to form am acidic oxide II. forms ionic chlorides III. has variable oxidation state IV. displaces hydrogen from dilute HCl.
A. I and III only
B. I and II only
C. II and IV only
D. I,II,III and IV
38. The electron configuration of carbon atom in its excited state is
A. $1s^2, 2s^2, 2p_x^2, 2p_y^0.$
B. $1s^2, 2s^2, 2p_x^1, 2p_y^1.$
C. $1s^2, 2s^1, 2p_x^1, 2p_y^1, 2p_z^1.$
D. $1s^1, 2s^2, 2p_x^1,2p_y^1, 2p_z^1.$
39. An oxide has the following properties. It I. is a white powder. II. reacts with HCl. III. reacts with NaOH. IV. is insoluble in water. The oxide is
A. alkaline
B. amphoteric
C. acidic
D. neutral
40. Which of the following statements about atoms of a metal is correct? They
A. readily accept electrons.
B. are soft.
C. are held together.
D. are held together by a sea of electron cloud.
Q41 See pages for figures
42. The atom with the electron cofiguratiom $1s^2s^22p^63s^23p^83d^{10}4s^24p^4$ is in
A. period 4, p-block
B. period 3, p-block
C. period 4, d block
D. period 3, d-block
43. Electropositivity of elements across the periodic table normally
A. remains constant down the group.
B. increases across the period.
C. decreases across the period.
D. decreases down the group.
44. See pages for figures
45. Which of the followiung oxides is amphoteric?
A. carbon(II)oxide
B. Nitrogen(IV)oxide
C. Lead(II)oxide
D. Calcium oxide
46. Which of the following processes occur during fractional distillation of petroleum?
A. Condensation and diffusion
B. Diffusion and evaporation
C. Diffusion and sublimation
D. Evaporation and condensatiion
47. If the molar mass of $X(HCO_3)^2$ is 162g mol-1, determine the relative atomic mass of X. [H = 1.0, C = 12.0, O = 16.0]
A. 40
B. 48
C. 61
D. 101
48. Charcoal is used in the decolourisation of sugar because of its
A. absorption property
B. amorphous property
C. oxidizing property
D. absorption property
49. The first definition of an element was made by
A. J. Dalton
B. A. Lavoisier
C. R. Boyle
D. J.J. Thompson
50. Which of the following scientists formulated the law of conservation of mass
A. A. Lavoisier
B. J. Dalton
C. R. Boyle
D. J. Proust
ANSWERS
1
A
21
B
41
C
2
B
22
D
42
A
3
A
23
C
43
C
4
D
24
A
44
B
5
C
25
D
45
C
6
C
26
B
46
D
7
C
27
A
47
A
8
D
28
B
48
D
9
C
29
C
49
C
10
B
30
A
50
A
11
D
31
C
12
C
32
B
13
D
33
B
14
B
34
C
15
C
35
C
16
B
36
B
17
B
37
C
18
C
38
C
19
C
39
B
20
D
40
D
