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Sekolah Menengah Kebangsaan St. MichaelChemistry Form 4 Chemical Equations

Drilling Exercise Set 1

Objective Questions

1. In an experiment , 1.12 g of metal X is burnt in oxygen o produce 1.6 g of metalX oxide.What is the empirical formula of metal x oxide ?[ Relative atomic mass : O, 16; X, 56 ]

A XO B XO2 C X2O D X2O3

2.

One compound has the percentage composition by mass as follow : Na , 36.5 %;S, 25.4%,

and 38.10% of oxygen.What is the empirical formula of this compound ?

[ Relative atomic mass, Na, 23; S, 32; O,16 ]

A Na2SO3 B Na2SO4 C Na2S2O3 D Na2S2O8

3. 2.43 g of an element X combines with 1.60g of another element.what is theempiricalformula for the resulting compound ?[ Relative atomic mass : X= 24.3 ; Y, 16 ]

A X2Y B XY C XY2 D X2Y3

4.24 g of an element T reacts with 32 g of sulphur to form a compound.What isthe mostlikely formula for this compound ?[ Relative atomic mass , T, 6; S, 32 ]

A TS B T2S C T3S4 D T4S

5. 0.25 moles of R combine with 12 g of oxygen to form an oxide.Which of thefollowing isthe empirical formula for the oxide of R ?

A R3O B RO3 C R2O3 D R3O2

6. A compound with the formula of R3T4 is formed by the reaction between 42.0 g ofR and 16.0 g of T . What is the relative atomic mass of R ?[ Relative atomic mass; T, 16 ]

A 14 B 32 C 42 D 56

7. What is the maximum quantity of iron that can be extracted from 116 g ofFe3O4 ?[ Relative atomic mass: O,16; Fe, 56 ]

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A 1.0 mole B 1.5 mole C 2.0 mole D 2.5 mole

8. A metal X forms a sulphate with the formula X2(SO4)3. What is the formula of thenitrate ofX ?

A XNO3 B X(NO3)3 C X3NO3 D X2NO3

9. 12.4 g of phosphorus reacts completely with 9.6 g of oxygen gas.Which of thefollowing isthe correct equation for the reactions ? [ P, 31 ; O, 16 ]

A P + O2 PO2B 3P + 2 O2 P3 O4

C 4P + 3 O2 2P2O3D 4P + 5 O2 2 P2O5

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The oxide for an element T has the formula T2O3 and its relative molecular massis 102.What is the relative atomic mass for T ?[ Relative atomic mass : O, 16 ]

A 18 B 27 C 36 D 50

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The heating reaction of potassium nitrate is represented by the equation below :

2 KNO3 2 KNO2 + O2

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What is the minimum volume of gas released when 1.01 g of potassium nitrateisheated at room condition ?[ Relative atomic mass: N, 14; O,16; K,39; 1 mol of gas occupies 24 dm3 at roomcondition]

A 0.06 B 0.12 C 1.2 D 2.4

With the presence of a catalyst, hydrogen peroxide decomposes according to theequation:

2 H2O2 2 H2 O + O2

If 4 moles of hydrogen peroxide is used, what is the volume of oxygen gasproduced at s.t.p?[1 mol of gas occupies 22.4 dm3 at s.t.p]A 22.4 dm3 B 30.8 dm3 C 40.4 dm3 D 44.8 dm3

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2 Ca + O2 2 CaO

4 g of calcium burns completely in air to form calcium oxide. Find the mass ofcalcium

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oxide produced. [ Ca, 40; O, 16 ]

A 1.6 g B 4.0 g C 5.6 g D 22.4 g

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4.2 g of element X reacts with 9.6 g of element Y to form a compound with thechemicalformula X2Y4. Given that the relative atomic mass of X is 14, find the relativeatomic massof Y.

A 4 B 8 C 16 D 3215

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Hydrated magnesium sulphate is heated according to the equation below :

MgSO4 . 7 H2O (s) MgSO4(s) + 7 H2O (g)

How many moles of water vapour is released when 54 g of magnesium sulphateis produced ?[ Relative atomic mass : Mg 24; O, 16; S, 32 ; H, 1 ]

A 0.45 mole B 4.5 mole C 3.15 mole D 6.3 mole

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2 Al (s) + 3 CuO (s) Al2O3 (s) + 3 Cu(s)

Find the mass of aluminium required to react completely with 24 g of copper(II)oxide.[ Relative atomic mass; O, 16; Al, 27 ; Cu, 64 ]

A 2.7 g B 5.4 g C 8.1 g D 10.8 g

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Write a balanced equation in the chemical formula for the reaction below :

Aluminium + Iron (III) oxide Aluminium oxide + Iron

A 2 Al (s) + Fe2O3(s) Al2O3 (s) + 2 Fe(s)B 2 Al (s) + Fe2O3(s) Al2O3 (s) + 2 Fe(g)C Al(s) + Fe2O3 (s) Al2O3 (g ) + 2 Fe(s)D 2 Al(s) + Fe2O3 (s) Al2O3 (s) + Fe (s)

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Ammonia gas is formed in Haber Process according to the chemical equationbelow :

N2 (g) + 3 H2 ( g) 2 NH3(g)

Calculate the volume of hydrogen needed to produced 100 cm3 of ammonia atroom conditions.[ Relative atomic mass : N, 14 ; H, 1 ; 1 mole of gas occupies 24 dm3 at roomconditions]

A 50 cm3 B 100 cm3 C 150 cm3 D 200 cm3

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Sodium hydrogen carbonate decomposes on heating according to the followingequation :

2 NaHCO3 (s) Na2CO3 (s) + CO2 (g) + H2 O (l)

If 10.0 g of sodium hydrogen carbonate is used, what is the mass of sodium

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carbonate that is produced ?[ Relative atomic mass : C, 12 ; O, 16 , Na, 23 ; H, 1 ]

A 6.4 g B 5.4 g C 5.0 g D 2.4 g

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Copper carbonate decomposes according to the equation below :

CuCO3(s) CuO(s) + CO2(g)If 24.8 g of copper carbonate is used, what is the volume of carbon dioxideproduced ?[1 mol of gas occupies 22.4 dm3 at s.t.p]A 5.24 dm3 B 2.24 dm3 C 3.48 dm3 D 4.48 dm3

Sekolah Menengah Kebangsaan St. MichaelChemistry Form 4 Chemical Equations

Drilling Exercise Set 1

Answer :

1. D2. A3. B4. D5. B6. D7. B

8. B9. C10. B11. B12. D13. C14. C15. C16. B17. A18. C

19. A20. D

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