Chemistry T5

8/12/2019 Chemistry T5

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Lesson 110: Paper 1

Name : _____________________________________

Class : _____________________________________

Date : _____________________________________

A. Multiple Choice Questions.

1. Both Chloride and calcium ions have the same(Proton number: Cl,17; Ca,20 )

A nucleon numberB number of neutronsC number of electronsD mass

2. How many elements are there in one molecule of ammonia?

A 1B 2C 3D 4

3. The proton number of element Y is 4. Which of the following statements are TRUEaboutatom Y.

I It has 4 electronsII It has 4 protonsIII Its electronic configuration is 2.2IV It is a Group IV element

A I, II, and III onlyB I, II and IV onlyC I, III and IV onlyD I, II, III and IV only


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4. Atom X has 16 protons and 21 neutrons in its nucleus. Which of the following symbolrepresents atom X?

A 16

37 X

B 37

16 X

C 36

17 X

D 21

16 X

5. Which of the following statement best explains that matter exists as tiny particles movingat random?

A A thin layer of oil is formed when an oil drop is placed on thesurface if water.

B When a perfume bottle is opened, the scent spreads to everypart of the room.

C Water cannot be easily compressed.D Large volume of steam is produced from a drop of boiling water.

6. In a neutral atom, the number of protons is equal to the

I number of neutrons.II number of electrons.III proton number.IV nucleon number.

A I and II onlyB I and III onlyC II and III onlyD I, II and IV only


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7. Which of the following industries need a chemist?

I Petroleum refineryII Plastic industryIII Food technologyIV Detergent manufacture

A I and II only

B II and III only

C I, II and III only

D I, II, III and IV

8.

Figure 1

Figure 1 shows the heating curve for naphthalene. At which stage does naphthalene existboth in a form of solid and liquid?

A P to QB Q to RC Above SD R to S


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9. Which of the following compounds has the correct relative formula mass?

[Relative Atomic Mass: H,1; C,12; N,14; O,16; Co,59; Cl,35.5; P,31; Ca,40]

A I and II only

B II and III only

C II and IV onlyD I and IV only

Compound Relative Formula MassI CoCl26H 2 O 238

II C18H27NO3 350

III Ca3(PO4)2 301

IV C16H10N2O2 262

10. Which of the following chemical formulae is correctly written?

Compound Chemical FormulaA Sodium oxide NaO

B Copper(II) nitrate CuNO3C Magnesium oxide Mg2OD Lead(II) chloride PbCl2

11. A molecular formula is a formula that shows the

A actual number of each atom of the elements in a moleculeB actual mass of a substance.C formula of a molecule of a substance that exists in solid state.D simplest ratio for the number of atoms of each type of element

in a molecule.


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12.

Figure 2

Figure 2 shows part of an apparatus used to determine the empirical formula of X oxide.Which of the following oxides can be X?

I Magnesium oxideII Lead(II) oxideIII Copper(II) oxideIV Calcium oxide

A I and II onlyB II and III onlyC III and IV onlyD I, II and III only

13. Which of the following chemical equations is balanced?

A CaCO3CaO + 2CO2

B Zn + HCl ZnCl2+ H2

C 2Mg + O2MgO

D CaCO3+ 2HNO3 Ca(NO3)2+ H2O + CO2

14. The relative molecular mass for substance MN2is 64. If the relative atomic mass of M is32, what is the relative atomic mass of N?

A 64

B 32C 16D 8


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15.

Figure 3

Figure 3 shows the set-up to conduct an experiment to study the effect of heat oncopper(II) carbonate. What is the expected observation?

A A blue residue is formed.B Limewater turns milky.C A green gas is released.D The copper(II) carbonate burns.

16. Which of the following has the same number of atoms with that found in 20 g of calcium?[Relative Atomic Mass: He, 4; Cl, 35.5; Ca, 40; Mg, 24; Li, 7]

A 12 g magnesiumB 0.5 mol chlorine gasC 0.25 mol of heliumD 1 mol lithium

17. Chemistry is defined as the study of

A weather changes.B collisions between two objects.C physical phenomena.D matter and the changes it undergoes.


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18. Which of the following statements is true about the changes in properties of elementsacross Period 3 of the Periodic Table?

A The elements become more electropositive.B The metallic property increases.C The number of electrons decreases.D The atomic radius decreases.

19. The proton number of phosphorus is 15. Where is phosphorus in the Periodic table?

A Group 5, Period 5B Group 15, Period 3C Group 13, Period 5D Group 15, Period 1

20.

Figure 4

Figure 4 shows the electron arrangement for atoms P, Q and R. Which of the followingstatements are true about the three atoms.

I They are not reactiveII They have low boiling pointsIII They do not lose electrons to other elementsIV They do not form molecules

A I, II and III onlyB I, II and IV onlyC I, III and IV onlyD I, II, III and IV


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21. Element Y is placed below element X in the same group in the Periodic Table.If the proton number of Y is 19, what is the electron arrangement for element X?

A 2.1B 2.7C 2.8.1D 2.8.8.1

22. What attitudes should be practiced by scientists in carrying out experiment?

I Systematic in planning the experiment.II Have analytical thinking.III Responsible about the safety of others.IV Honest and accurate in recording data.

A I and II onlyB II, III and IV onlyC I, II and III onlyD I, II , III and IV

23. Sodium oxide has a high melting point because

A the attraction forces between its particles are very strong.B it has large mass.C it is soluble in water.

D it is in crystal state.

24. What happens at the particulate level when sodium metal reacts with chlorine gas?

A Chlorine atom donates one proton to sodium atom.B Chlorine atom accepts one electron from sodium atom.C Sodium atom and chlorine atom shares one electron.D Sodium atom receives an electron from chlorine atom.


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25. How many electrons are shared by carbon and chlorine atoms in tetrachloromethanemolecule, CCl4?

A 4B 5C 8D 10

26. Electrolytes produce _______ when dissolved in water.

A atomsB ionic compoundsC gas bubblesD ions

27. What is the disadvantage of using mercury cell?

A Not long lastingB HeavyC Current and voltage provided is not fixedD Cannot be recharged

28.

Figure 5

In figure 5 what would be formed at the copper plate after some time?

A Hydrogen gasB Copper(II) ionsC Magnesium metalD Copper metal


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29. Which of the following methods is used in manufacturing chlorine?

A Boiling sodium chloride solution.B Electrolysis of molten sodium chloride.C Heating solid sodium chloride.D Neutralisation of hydrochloric acid with sodium hydroxide.

30. Which of the following electrolytes is used in the industrial extraction of aluminium?

A Impure bauxite and cryolite.B Aluminium oxide and aluminium.C Aluminium oxide and cryolite.D Aqueous solution of aluminium oxide.

31.

Figure 6

Which of the following substances will make the bulb glow brighter when added to thewater in the beaker?

A EthanolB TetrachloromethaneC GlucoseD Hydrochloric acid


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32. Which of the following statements is NOTtrue about the electroplating process of an ironring with nickel?

A Direct current is used.B Iron ring is the anode.C Aqueous nickel(II) sulphate solution is used as electrolyte.D To get an even plating, low current is used.

33. Which of the following is the first step in a scientific investigation?

A Suggesting a hypothesis.B Making an inference.C Identifying a problem.D Identifying variables.

34. A strong acid ________

A cannot conduct electricity.B reacts vigorously with water.C dissociates completely in water.D dissolves slightly in water.

35. Which of the following is NOT true about alkali?

A Reacts with acid to produce salt and water.B Its pH value is more then 7.C It turns red litmus paper blue.D Reacts with metal oxide to produce oxygen gas.

36. Which of the followingsolutions has the highest pH value?

A 0.01 mol dm-3

of hydrochloric acidB 0.01 mol dm

-3of ethanoic acid

C 0.01 mol dm-3

of potassium hydroxide

D 0.01 mol dm-3

of ammonia solution


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37. Which of the following substances will produce a solution with pH value of 7 whendissolved in water?

A Sodium oxideB EthanolC Sulphur dioxideD Carbon dioxide

38. Calculate the mass of sodium hydroxide needed to prepare 500 cm3of 0.5 mol dm

-3

ofsodium hydroxide solution?

(Relative Atomic Mass: H,1; O,16; Na,23)

A 14.3 gB 10.0 gC 15.8 gD 40.0 g

39. The following chemical equation shows the neutralisation reaction between sulphuricacid and sodium hydroxide:

H2SO4+ 2NaOHNa2SO4+ 2H2O

Calculate the volume of 0.4 mol dm-3

of sodium hydroxide required to neutralise 50.0 cm3

of 0.2 mol dm-3

of sulphuric acid.

A 30.0cm3B 35.0 cm

3

C 40.0 cm3

D 50.0 cm3

40. Sulphuric acid is a diprotic acid because

A it can react as an acid and also as a dehydrating agent.B it contains H

+and OH

-ions.

C it produces two moles of H+

ions from one mole of acid in water.D it contains H

2+ions.


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41. Which of the following compound forms an acidic solution when dissolved in water?

A Carbon dioxideB Magnesium oxideC TetrachloromethaneD Copper(II) oxide

42. Which of the following salts can be prepared by double decomposition reaction?

A Lead(II) sulphateB Lead(II) nitrateC Copper(II) sulphateD Ammonium nitrate

43. A white precipitate is formed when dilute hydrochloric acid is added to solution X. Whichof the following is likely to be X?

A Silver nitrateB Ammonium nitrateC Barium nitrateD Zinc nitrate

44. Excess magnesium is reacted with 0.1 mol of hydrochloric acid. What is the volume of

hydrogen gas liberated at room temperature?(1 mole of gas occupies 24 dm

3at room temperature)

A 2400 cm3

B 1200 cm3

C 600 cm3

D 0.05 cm3

45. Which of the following materials is used to build aeroplanes?

A Aluminium

B Stainless steelC ZincD Duralumin


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46. Which of the following processes takes place during the Contact Process?

A Sulphur trioxide is liquefied under pressure.B Sulphur dioxide is dissolved in water.C Sulphur trioxide is dissolved in concentrated sulphuric acid.D Sulphur dioxide is dissolved in concentrated sulphuric acid.

47. Which of the following statements are true about the Haber Process?

I The ratio of hydrogen to nitrogen is used 3: 1.II The process is carried out at 1 atmospheric pressure.III Vanadium(V) oxide is used as catalyst.IV The optimum temperature is 500 C.

A I and II onlyB I, II and III onlyC I and IV onlyD II, III and IV only

48. In Haber Process, the ammonia produced is separated from both the hydrogen andnitrogen gas by

A SynthesisB CoolingC Condensation

D Boiling

49. Glass is a different material from ceramics because glass

A can be recycled.B is chemically inert.C is used as heat insulators.D is used as electric insulators.


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50. Alloys are harder than pure metals because the atoms in alloy are

A held closer together.B arranged closer together.C able to vibrate easily.D not able to slide easily over its layers.

51. Which of the following substances undergo sublimation?

I BromineII IodineIII Solid carbon dioxideIV Solid Argon

A I and III onlyB II and III onlyC II, III and IV onlyD I, III and IV only

52.The melting and boiling points of X and Y are shown in Table 1.

Table 1

What are the states of X and Y at room temperature?

X Y

A Liquid liquidB Solid LiquidC Liquid solidD solid solid

Melting Point/C Boiling Point/C

X -20 52Y 45 300


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53. Which of the following occurs when solid CO2sublimes to gaseous CO2?

A There is loss in kinetic energy.B The CO2molecules become lighter.C The attractive forces between CO2molecules become weaker.D CO2molecules react with oxygen in the atmosphere.

54.

Figure 7

Figure 7 shows a cooling curve of liquid X. Which of the following statements are TRUE?

I At QR, X exists as solid and liquid.II At PQ, X absorbs heat.

III At RS, X is a solid.IV The melting point of X is 80C.

A I and III onlyB I, II and III onlyC I, II and IV onlyD I, III and IV only

55. The most suitable apparatus for measuring accurately 30.00 cm3of a solution is a

A burette

B measuring cylinderC beaker

D pipette


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56. Which of the following statements are true about isotopes?

I Isotopes are atoms of the same element.II Isotopes have different chemical properties.III Isotopes have different physical properties.IV Isotopes have different numbers of neutrons and electrons.

A I and II onlyB I and III onlyC I, II and IV onlyD I, III and IV only.

57.

Table 2

Table 2 shows the proton number and nucleon number of elements W, X, Y and Z.Which of the following pairs of elements are isotopes?

A W and XB X and ZC W and Y

D W and Z

Element Proton Number Nucleon NumberW 8 18X 9 16

Y 7 18Z 8 16


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58. Y is a compound consists of positive and negative ions. At room temperature, it exists asa solid. Which of these are the properties of compound Y?

I Good electrical conductor in molten stateII Dissolves in organic solventIII High melting and boiling pointIV Volatile

A I and III onlyB II and III onlyC II and IV onlyD III and IV only

59. How many times is one atom of calcium heavier than one moleculeof oxygen?[Relative Atomic Mass: Ca,40; O,16]

A 2/5B 4/5C 5/4D 5/2

60. Calculate the maximum mass of iron that can be extracted from 200 kg of iron(III) oxide,Fe2O3.[Relative Atomic Mass: Fe,56; O,16]

A 100 kgB 133 kgC 140 kgD 160 kg


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61. What is the number of sodium ions present in 20 g of sodium oxide?[Relative atomic mass: Na;23, O;16; Avogadro constant: 6X10

23mol

-1]

A 20 x 6 x 1023

x 23

B 20 x 6 x 1023

x 23 x 62

C 20 x 6 x 1023

x 262

D 20 x 6 x 1023

x 2

62. How many moles of atoms are present in 3 g of ethanoic acid, CH 3COOH?[Relative Atomic Mass: C,12; H,1; O,16]

A 0.3B 0.4C 0.2D 0.5

63. Which of the following samples of gases occupy the samevolume as 7.1 g of chlorine gas at STP?[Relative Atomic Mass: H,1; Ar,40; O,16; C,12; Cl,35.5; Molar volume of gas: 22.4dm

3at

STP]

I 0.1 g of hydrogen gas

II 3.2 g of oxygen gasIII 4.4 g of carbon dioxideIV 4.0 g of argon gas

A I, II and IIIB I, II and IVC I, III and IVD II, III and IV


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64. 7.14 g of an oxide of metal X contains 5 g of metal X. Calculate the empirical formula ofthis metal oxide.

[Relative Atomic Mass: X,56; O,16]

A X3O4B X2O3C XOD X2O5

65. The empirical formula of a metal oxide is Y2O5. The oxide contains 44% of metal Y bymass. What is the relative atomic mass of Y?[Relative Atomic Mass: O,16]

A 13B 31C 63D 157

66. Magnesium reacts with excess hydrochloric acid in a beaker. Calculate the volume ofhydrogen gas evolved under STP when 1.2 g of magnesium is used.[Relative Atomic Mass: Mg, 24; Molar volume of gas: 22.4 dm

3at STP]

A 1.12 cm3

B 2.24 cm3

C 112 cm3

D 1120 cm3


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67.

Figure 8

The letter P,Q,R,S and T are place in figure 8 represents element in the Periodic Table .Which two can act as catalyst?

A P and QB P and RC Q and SD S and T

P R T

Q S

68. The electron arrangement for atom X is 2.8.8.1. Based on this information, it can bepredicted that

I X reacts vigorously with water.

II X reacts with chlorine gas to form a white compound.III X burns in air to form a compound with formula X2O.IV X is more electropositive than sodium.

A I, II and IIIB I, II and IVC I, III, and IVD I, II, III and IV


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73. J is an element in Group 13 and M is an element in Group 16 of thePeriodic Table. When J and M react with each other, the most likely

chemical formula for the product formed is

A J2M3B J3M2C JMD J3M6

74. Both potassium ion and chloride ion have the same[Proton number: K,19; Cl,17]

A number of protonsB number of electronsC number of neutronsD number of isotopes

75. X is a compound which does not conduct electricity either in the solid state or in themolten state. The possible pairs of elements that have chemically reacted to formcompound X are

I Lead and bromineII Nitrogen and hydrogenIII Chlorine and oxygenIV Calcium and oxygen

A I and II onlyB II and III onlyC I, II and IV onlyD II, III and IV only


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76. Which of the following experiments will produce oxygen and hydrogen gas at theelectrodes?

Electrolysis ExperimentsElectrolyte Electrodes

A Copper sulphate solution Copper

B Molten sodium chloride PlatinumC Concentrated potassium chloride solution Carbon

D Calcium nitrate solution Platinum

77.

Figure 9

Figure 9 shows the set up of apparatus for the electrolysis of molten lead(II) chlorideusing carbon electrodes. Which of the following statements are TRUE?

I Lead(II) ion accepts two electrons to form lead atomII The gas produced at the cathode is yellowish green in colour.III Lead(II) chloride can only conduct electricity in the molten state.IV Chloride ion donates one electron to form chlorine atom.

A I, II and IIIB I, II and IVC I, III, and IVD II, III and IV


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78. Which of the following products are formed during the electrolysis of diluteaqueous copper(II) chloride solution using carbon electrodes?

Anode CathodeA Oxygen gas is released Copper is depositedB Oxygen gas is released Hydrogen gas is releasedC Hydrogen gas is released Copper is depositedD Chlorine gas is released Hydrogen gas is released

79. Which of the following sets of electrodes and electrolyte used inelectroplating a coin with nickel?

Anode Cathode Electrolyte

A Coin Nickel Copper(II) sulphateB Coin Nickel Nickel(II) sulphate

C Nickel Coin Nickel(II) sulphate

D Nickel Coin Copper(II) sulphate


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80.

Figure 10

Figure 10 shows the apparatus for the purification of copper by electrolysis. Which of the

following statements are TRUE?

I The impure copper is cathode.II The colour of the copper(II) sulphate solution remains the same.III The pure copper electrode becomes thicker.IV Copper(II) sulphate solution can be substituted with copper(II)

nitrate solution

A I, II and IIIB I, II and IVC I, III, and IVD II, III and IV

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Chemistry T5