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I. PROPORTIONS IN CHEMICAL COMPOUNDS (2)
True (T) or false (F) [2]:
1. The law of definite proportions proves that CO2 and CO both decompose to produce the same weight of carbon and oxygen. _______________
2. Joseph Proust stated that a specific compound always contains the same elements in definite proportions by mass. _______________
II. THE CHEMICAL MOLE (30)
Calculate the number of molecules in 20.05 g of P2S5 (s) [3] :
Calculate the mass of 2.893 x 1020 molecules of BF3 (g) [3] :
Calculate the number of moles in 15.0 g of CaO(s) [3] :
Calculate the number of copper ions found in 13.7 moles of chalcocite (Cu2S (s)) [3] :
Calculate the mass of 20.00 mL of O2 (g) at STP [3] :
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Calculate the moles of iodine atoms in 2.00 L of hydrogen iodide (HI (g)) at SATP [3]
:
Calculate the mass of 1.27 x 1024 molecules of sodium orthoperiodate (Na5IO6 (aq)) [3] :
Calculate the moles of bromine vapour (Br2 (g)) in 72.48 kg [3] :
Calculate the moles of chloride ions found in 7.894 moles of PbCl4 (s) [3] :
Calculate the mass of galena (PbS2 (s)) required to produce 4.96 x 1023 sulfide ions [3] :
III. PERCENTAGE COMPOSITION (20)
Calculate the percentage composition of soda ash (Na2CO3) from its formula [3] :
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In an experiment, 6.900g of sodium metal reacted with 10.66g of chlorine gas to give 17.56g of sodium chloride. Calculate the percentage composition of table salt (NaCl) from empirical data [3] :
When a 6.00g sample of an organic compound (CXHXOX) was completely combusted, 2.34g of water and 5.74g of carbon dioxide were produced. Calculate the percentage composition of this compound [4] :
Calculate the percentage composition of chloromycetin (C11H12N2O5Cl2) [3] :
Calculate the weight of chlorine that can be obtained from the decomposition of
100.0g of calcium chloride (CaCl2) [3] :
A 24.00g sample of a mixture of KClO3 and KCl is heated until all the oxygen is removed. The product, completely KCl, weighs 18.00g. Calculate the percentage of
KClO3 in the original mixture [4] :
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IV. EMPIRICAL & MOLECULAR FORMULAE (22)
What do the subscripts in a formula represent [1] ? ____________________
Indicate whether the following formulas are empirical (E) or molecular (M) [5] :
CH4 SO2 CH2O C6H12O6 Na2O2
____________________ ____________________ ____________________ ____________________ ____________________
233.7g of aluminum react with 417.0g of sulfur. Determine the empirical formula for the compound [3] :
A compound contains 82.5% carbon and 17.5% hydrogen. Determine the empirical formula for the compound [3] :
Titanium(_) chloride (TiClX) is converted into 2.40g of TiO2 and 12.9g of AgCl. Determine the empirical formula for the original compound [3] :
The percentage composition of a compound is 5.9% hydrogen and 94.1% oxygen. Determine the molecular formula for the compound if its weight is 34g/mol [3] :
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The simplest formula of 1,2-dibromoethane, a colourless liquid with a sweet odour
and manufactured synthetically by the reaction of ethylene with bromine, is CH2Br. Determine the molecular formula for the compound if its molar mass is 187.86g/mol [4] :
V. BALANCING CHEMICAL EQUATIONS (20)
Balance the following equations [20] :
1. SiCl4 (l) + H2O (l) SiO2 (s) + HCl (aq)
2. As (s) + NaOH (aq) Na3AsO3 (s) + H2 (g)
3. Au2S3 (s) + H2 (g) Au (s) + H2S (g)
4. V2O5 (s) + HCl (aq) VOCl3 (aq) + H2O (l)
5. Hg(OH)2 (aq) + H3PO4 (aq) Hg3(PO4)2 (aq) + H2O (l)
6. SiO2 (s) + HF (g) SiF4 (g) + H2O (l)
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7. Zn(s) + HCl (aq) ZnCl2 (s) + H2 (g)
8. HClO4 (aq) + P4O10 (s) H3PO4 (aq) + Cl2O7 (aq)
9. N2 (g) + O2 (g) + H2O (l) HNO3 (aq)
10.NH4NO3 (s) N2 (g) + O2 (g) + H2O (l)
VI. GRAVIMETRIC STOICHIOMETRY (31)
The average human requires 120.0 grams of glucose (C6H12O6) per day. How many
grams of CO2 (in the photosynthesis reaction) are required for this amount of glucose? The photosynthetic reaction is [3] :
6 CO2 (g) + 6 H2O (l) C6H12O6 (aq) + 6 O2 (g)
Silver sulfide (Ag2S) is the common tarnish on silver objects. What weight of silver
sulfide can be made from 1.23 mg of hydrogen sulfide (H2S) obtained from a rotten egg? The reaction of formation of silver sulfide is given below, however, the equation must first be balanced [5] :
Ag(s) + H2S(g) + O2(g) Ag2S(s) + H2O(l)
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Given the following equation: 2 C4H10 (g) + 13 O2 (g) 8 CO2 (g) + 10
H2O (l) , show what the following molar ratios should be [5] :
a. C4H10 / O2
b. O2 / CO2
c. O2 / H2O
d. C4H10 / CO2
e. C4H10 / H2O
Given the following equation: 2 K(s) + Cl2 (aq) 2 KCl (aq) :
a) How many grams of KCl are produced from 2.50 g of K and excess Cl2? [3]
b) From 1.00 g of Cl2 and excess K? [3]
Given the following equation: Na2O(s) + H2O (l) 2 NaOH (aq)
a) How many grams of NaOH are produced from 1.20 x 102 grams of Na2O? [3]
b) How many grams of Na2O are required to produce 1.60 x 102 grams of NaOH? [3]
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Given the following equation: Cu (s) + 2 AgNO3 (aq) Cu(NO3)2 (aq) + 2 Ag
(s)
a) How many moles of copper are needed to react with 3.50 moles of silver nitrate? [3]
b) If 89.5g of silver were produced, how many grams of copper reacted? [3]
VII. NOMENCLATURE (70)
Give the correct name of the following compounds [15] :
1. HBr (aq) ______________________________
2. CoSO2 ______________________________
3. Ni2(CO4)3 ______________________________
4. KO2 ______________________________
5. Ba3(PO3)2 ______________________________
6. SO3 ______________________________
7. RbOH ______________________________
8. SnH4 ______________________________
9. Hg(VO2)2 ______________________________
10.PbC ______________________________
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11.Au(C2H3O2)3______________________________
12.NH4ClO4 ______________________________
13.H2CrO4 ______________________________
14.Na2O2 ______________________________
15.LiNO3 • 12H2O ______________________________
Name the following polyatomic ions [5] :
1. SO42- ____________________
2. C2H3O2- ____________________
3. NO3- ____________________
4. NH4+ ____________________
5. PO43- ____________________
What is the difference between HCN(g) and HCN(aq) in terms of nomenclature [2] ?
____________________________________________________________________________________________________________________________________________________________
Give the correct chemical formula of the following compounds [15] :
1. Ammonium Acetate ______________________________
2. Hydrogen Peroxide ______________________________
3. Nitrous Acid ______________________________
4. Strontium Sulfite Octahydrate ______________________________
5. Chromium(VI) Orthohypoaresnite ______________________________
6. Chromium(II) Metaperarsenate ______________________________
7. Tin(IV) Oxide ______________________________
8. Diphosphorus Pentachloride ______________________________
9. Titanium(II) Pertitanate ______________________________
10.Gold(III) Hypostannite ______________________________
11.Thallium Carbide ______________________________
12.Cobalt(III) Selenide ______________________________
13.Chlorine gas ______________________________
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14.Iron(III) Carbonate ______________________________
15.Disulfur Tetroxide ______________________________
Explain why F3N is not a correct chemical formula [1] :
____________________________________________________________________________________________________________________________________________________________
Give two valences of the following multivalent metals [16] :
1. lead _____ _____
2. nickel _____ _____
3. mercury _____ _____
4. gold _____ _____
5. iron _____ _____
6. tin _____ _____
7. cobalt _____ _____
8. copper _____ _____
Give the IUPAC name for sulfuric acid (H2SO4 (aq)) [1] :
____________________________________
Fill in the missing blanks [8] :
Type Formula Name
MONOVALENT BINARY IONIC COMPOUND LiBr(s) _________________________
MULTIVALENT BINARY IONIC COMPOUND ____________ Copper(II) Chloride
TERTIARY IONIC COMPOUND Na3PO4 (aq) _________________________
HYDRATED COMPOUND ____________Copper(II) Sulfate Pentahydrate
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MOLECULAR COMPOUND H2S _________________________
BINARY ACID ____________ Hydrofluoric Acid
OXYACID HClO4 (aq) _________________________
BASIC COMPOUND (BASE) ____________Aqueous Sodium Hydroxide
Give the formula for the following polyatomic ions [5] :
1. thiosulfate ____________________
2. hydroxide ____________________
3. carbonate ____________________
4. cyanide ____________________
5. chlorate ____________________
Fill in and name the cation that will complete this acid reaction chemical equation [2] :
HNO3 (aq) + H2O(l) NO3- (aq)
+ ________ (aq)
Cation: ____________________
>99%
