Name: _____________________
Period: ___
Scientific Measurement
(1) Change the number in standard form into scientific notation.
(a) 340000
(b) 0.00156
(c) 28900000
(d) 0.0000084
(2) Change the number in scientific notation to standard form.
(c) 9.4x107
(d) 4.2x10-4
(a) 5.61x104 (b) 7.82x10-6
(3) Complete the following metric conversions:
(a) 58 mL = ___________ L
(b) 0.0065 s = ___________ µs
(c) 840 km = ___________ Mm
(d) 0.046 mg = ___________ ng
(4) The distance from Los Angeles to New York is 2833 miles. What is the distance in km? (1 mile = 1.6093 km)
(5) A car has a mass of 2200 kg.
(a) What is the mass in pounds? (1 kilogram = 2.2046 pounds)
(b) What is the mass in tons? (1 ton = 2000 pounds)
(c) What is the mass in metric tons? (1 metric ton = 1000 kg)
(6) A box has a volume of 250 cm3.
(a) What is the volume in m3?
(b) What is the volume in in3? (1 inch = 2.54 cm)
(7) The speed limit reads 70 miles/h.
(a) What is the speed in km/h?
(b) What is the speed in m/s?
(8) Complete the following temperature conversions:
(a) 80 °C = _____ F = _____ K
(b) _____ °C = -40 F = _____ K
(c) _____ °C = _____ F = 300 K
(9) Give the number of significant figures in each value.
(a) 45 (b) 0.016 (c) 205 (d) 0.01200 (e) 2.2x105
(f) 300.
(10) Round each value to the number of significant figures indicated.
(a) 1.26 (2) (b) 0.01242 (3) (c) 4565 (2) (d) 4.596x103 (3)
(e) 22.556 (3)
(f) 0.0012448 (3)
(11) Complete each operation. Give the answer to the correct number of significant figures.
(a) 2.15 x 8.2 (b) 14.153 + 2.35 (c) 18.62 ÷ 1.24 (d) 4.86 - 1.4 (e) 5.65 x 10.21 ÷2.4
(f) 18.25 + 3.435 - 2.1
Density
(1) A metal coin has a mass of 25.5 g. When the coin is place in a graduated cylinder with 25.00 mL of water, the water level
rises to 26.32 mL. What is the density of the coin?
(2) The most dense naturally occurring substance on earth is the element iridium (22.65 g/cm3). What is the mass of a block of
iridium with dimensions 3.45 cm by 2.84 cm by 1.15 cm? What is the mass in kg?
(3) An empty container has a mass of 1025 g. When the container is filled 825 mL of gasoline the mass of the container and the
gasoline is 1630 g. What is the density of gasoline in g/mL? What is the density in kg/m3?
(4) Due to increased global temperatures, about 50 km3 of ice from the glaciers of Greenland melts each year. Given that ice has
a density of 917 kg/m3, determine the mass of ice that melts each year in kg. What volume of water (density = 1000 kg/m3) is
added to the ocean every year from this glacial melt in m3? What is the volume in km3?
Atomic Structure
(1) Determine the number of protons and electrons in each of the following elements/ions.
(d) Br(a) S
(b) Ne
(c) Ca2+
(2) Give the number of protons, electrons, and neutrons of each of the following elements/ions.
222
(a) 86 Rn
(b)
14
6
C
59
(c) 27 Co
2+
(e)
15
7
N 3-
(3) Silicon has three isotopes: Silicon-28 (exact mass = 27.97693, abundance = 92.21%), Silicon-29 (exact mass = 28.97649,
abundance = 4.70%), and Silicon-30 (exact mass = 29.97376, abundance = 3.09%).
(a) Determine the number of neutrons of each isotope.
(b) Determine the average atomic mass of Silicon.
(4) Boron has two isotopes: Boron-10 (exact mass = 10.01294) and Boron-11(exact mass = 11.00930).
(a) Determine the number of neutrons of each isotope.
(b) From the periodic table, what is the average atomic mass of boron?
(c) Determine the abundance of each isotope. (Hint: what should the to abundances add up to?)
Answers:
Scientific Measurement
(2) (a) 56100 (b) 0.00000782 (c) 94000000 (d) 0.00042
(1) (a) 3.4x105 (b) 1.56x10-3 (c) 2.89x107 (d) 8.4x10-6
(3) (a) 0.058 L (b) 6500 µs (c) 0.84 Mm (d) 46000 ng
(4) 4559 km
(5) (a) 4850 pounds (b) 2.452 tons (c) 2.200 metric tons
(6) (a) 0.000250 m3 (b) 15.3 in3
(7) (a) 113 km/hour (b) 31.3 m/s
(8) (a) 176 F 353 K (b) -40 ºC 233 K (c) 27 ºC 80.6 F
(9) (a) 2 (b) 2 (c) 3 (d) 4 (e) 2 (f) 3
(10) (a) 13 (b) 0.0124 (c) 4.6x103 (d) 4.60x103 (e) 22.6 (f) 0.00124
(11) (a) 18 (b) 16.50 (c) 15.0 (d) 3.5 (e) 24 (f) 19.6
Density
(1) 19.3 g/mL
(2) 255 g 0.255 kg
(3) 0.733 g/mL 733 kg/m3
13
10
(4) mass = 4.6x10 kg ice/water volume = 4.6x10 m3 46 km3
Atomic Structure
(1) (a) 16 p 16 e (b) 10 p 10 e (c) 20 p 18 e (d) 35 p 36 e
(2) (a) 86 p 86 e 136 n (b) 6 p 6 e 8 n (c) 27 p 25 e 32 n (d) 7 p 10 e 8 n
(3) (a) 14 n, 15 n, and 16 n (b) 28.09 amu
(4) (a) 5 n and 6 n (b) 10.811 (c) boron-10 (19.9%) and boron-11
(80.1%)
Name: _____________________
Period: ___
Chemical Compounds
(1) Name the following ionic compounds:
1. KCl
2. CuBr2
3. Cs3PO4
4. MoC2O4
5. BeSO3
6. Mg(NO3)2
7. V2O3
8. Ba(IO3)2
9. AlCl3
10. HgS
11. CrO
12. AuCl3
13. LiHCO3
14. PbI2
15. MnO2
16. NaBrO3
17. Zn(IO2)2
18. Sr(OCN)2
19. CoC2O4
20. AgCl
21. Li3PO4
22. CdI2
23. CaF2
24. Fe2O3
25. Cr2S3
26. Ti(HPO4)2
27. KMnO4
28. Ba(HSO3)2
29. RbBr
30. PbS2
(2) Write the formula for the following ionic compounds:
1. cesium fluoride
2. copper (II) sulphate
3. calcium carbonate
4. zinc cyanide
5. palladium (IV) chloride
6. iron (III) phosphate
7. sodium oxalate
8. cobalt (III) fluoride
9. potassium periodate
10. aluminum sulphite
11. beryllium chromate
12. manganese (II) hypobromite
13. gallium chlorate
14. barium hydroxide
15. ammonium chloride
16. copper (II) acetate
17. titanium (IV) oxide
18. magnesium bromide
19. iron (II) cyanide
20. lithium borate
21. calcium phosphide
22. potassium thiocyanate
23. nickel (II) chloride
24. sodium hydrogen sulphate
25. ammonium sulphate
26. cadmium sulphide
27. tin (IV) phosphite
28. silver nitrate
29. cesium dihydrogen phosphate
30. lead (IV) sulphide
(3) Name the following acids:
1. HBr
2. HNO2
3. HClO3
4. H2CO3
5. HC2H3O2
6. HCl
7. H3PO4
8. HBrO2
9. HSCN
10. HClO
(4) Write the formula for the following acids:
1. sulphuric acid
2. hydrofluoric acid
3. iodous acid
4. bromic acid
5. sulphurous acid
6. hydroiodic acid
7. chlorous acid
8. nitric acid
9. oxalic acid
10. hydrocyanic acid
(5) Name the following covalent compounds:
1. CS2
2. Si3N4
3. PBr5
4. SF6
5. P2F4
6. PCl5
7. CI4
8. N2O4
9. IF7
10. BN
11. B5H9
12. SiS2
13. P4O10
14. CO
15. NCl3
16. ClO2
(6) Write the formula for the following covalent compounds:
1. silicon dioxide
2. carbon tetrabromide
3. tetraiodide nonoxide
4. disulphur decafluoride
5. chlorine pentafluoride
6. phosphorus tribromide
7. sulphur tetrachloride
8. diiodide tetroxide
9. iodine monobromide
10. nitrogen triodide
11. dinitrogen pentoxide
12. oxygen difluoride
13. tricarbon dioxide
14. sulphur tetrafluoride
15. dichlorine heptoxide
16. tetraphosphorus decasulphide
(7) Name the following compounds:
1. MgBr2
2. FeO
3. K3PO4
4. NF3
5. Ni(ClO3)2
6. HIO3
7. S3Cl2
8. BeBr2
9. MoCl2
10. BaCO3
11. Cr(IO3)3
12. HgO
13. Li3AsO3
14. Br2O
15. H2CrO4
16. Ca(IO)2
17. S2O
18. NaOCN
19. PbSiO3
20. H3PO3
21. CsCl
22. Al(BrO4)3
23. PI3
24. Mn(HCO3)2
25. Mg(HSO4)2
26. LiClO
27. VI3
28. N2F2
29. HBrO
30. SrHPO4
(8) Write the formula for the following compounds:
1. lithium iodide
2. potassium thiosulphate
3. carbonous acid
4. nickel (III) chloride
5. bromine pentafluoride
6. calcium bromite
7. chromium (II) oxalate
8. silver acetate
9. zinc phosphate
10. molybdenum (II) fluoride
11. perchloric acid
12. strontium hypoiodite
13. cesium carbonite
14. diboron hexafluoride
15. magnesium cyanide
16. ammonium nitrate
17. sodium permanganate
18. hypoiodous acid
19. barium hydrogen sulphate
20. iron (II) fluoride
21. aluminum arsenate
22. cobalt (III) acetate
23. sulphur trioxide
24. titanium (IV) bromide
25. zinc hydrogen carbonite
26. boric acid
27. copper (II) carbonate
28. lithium dihydrogen phosphite
29. trisilicon tetranitride
30. magnesium silicate
Answers:
(1)
1. potassium chloride
2. copper (II) bromide
3. cesium phosphate
4. molybdenum (II) oxalate
5. beryllium sulphite
6. magnesium nitrate
7. vanadium (III) oxide
8. barium iodate
9. aluminum chloride
10. mercury (II) sulphide
11. chromium (II) oxide
12. gold (III) chloride
13. lithium hydrogen carbonate
14. lead (II) iodide
15. manganese (IV) oxide
16. sodium bromate
17. zinc iodite
18. strontium cyanate
19. cobalt (II) oxalate
20. silver chloride
21. lithium phosphate
22. cadmium iodide
23. calcium fluoride
24. iron (III) oxide
25. chromium (III) sulphide
26. titanium (IV) hydrogen phosphate
27. potassium permanganate
28. barium hydrogen sulphite
29. rubidium bromide
30. lead (IV) sulphide
(2)
1. CsF
2. CuSO4
3. CaCO3
4. Zn(CN)2
5. PdCl4
6. FePO4
7. Na2C2O4
8. CoF3
9. KIO4
10.Al2(SO3)3
11. BeCrO4
12. Mn(BrO)2
13. Ga(ClO3)3
14. Ba(OH)2
15. NH4Cl
16. Cu(C2H3O2)2
17. TiO2
18. MgBr2
19. Fe(CN)2
20. Li3BO3
21. Ca3P2
22. KSCN
23. NiCl2
24. NaHSO4
25. (NH4)2SO4
26. CdS
27. Sn3(PO4)4
28. AgNO3
29. CsH2PO4
30. PbS2
1. hydrobromic acid
2. nitrous acid
3. chloric acid
4. carbonic acid
5. acetic acid
6. hydrochloric acid
7. phosphoric acid
8. bromous acid
9. hydrothiocyanic acid
10. hypochlorous acid
1. H2SO4
2. HF
3. HIO2
4. HBrO3
5. H2SO3
6. HI
7. HClO2
8. HNO3
9. H2C2O4
10. HCN
(3)
(4)
(5)
1. carbon disulphide
2. trisilicon tetranitride
3. phosphorus pentabromide
4. sulphur hexafluoride
5. diphosphorus tetrafluoride
6. phosphorus pentachloride
7. carbon tetraiodide
8. dinitrogen tetroxide
9. iodine heptafluoride
10. boron mononitride
11. pentaboron nonahydride
12. silicon disulphide
13. tetraphosphorus decoxide
14. carbon monoxide
15. nitrogen trichloride
16.chlorine dioxide
1. SiO2
2. CBr4
3. I4O9
4. S2F10
5. ClF5
6. PBr3
7. SCl4
8. I2O4
9. IBr
10. NI3
11. N2O5
12. OF2
13. C3O2
14. SF4
15. Cl2O7
16. P4S10
1. magnesium bromide
2. iron (II) oxide
3. potassium phosphate
4. nitrogen trifluoride
5. nickel (II) chlorate
6. iodic acid
7. trisulphur dichloride
8. beryllium bromide
9. molybdenum (II) chloride
10. barium carbonate
11. chromium (III) iodate
12. mercury (II) oxide
13. lithium arsenite
14. dibromine monoxide
15. chromic acid
16. calcium hypoiodite
17. disulphur monoxide
18. sodium cyanate
19. lead (II) silicate
20. phosphorous acid
21. cesium chlorde
22. aluminum perbromate
23. phosphorus triiodide
24. manganese (II) hydrogen carbonate
25. magnesium hydrogen sulphate
26. lithium hypochlorite
27. vanadium (III) iodide
28. dinitrogen difluoride
29. hypobromous acid
30. strontium hydrogen phosphate
1. LiI
2. K2S2O3
3. H2CO2
4. NiCl3
5. BrF5
6. Ca(BrO2)2
7. CrC2O4
8. AgC2H3O2
9. Zn3(PO4)2
10. MoF2
11. HClO4
12. Sr(IO)2
13. Cs2CO2
14. B2F6
15. Mg(CN)2
16. NH4NO3
17. NaMnO4
18. HIO
19. Ba(HSO4)2
20. FeF2
21. AlAsO4
22. Co(C2H3O2)3
23. SO3
24. TiBr4
25. Zn(HCO2)2
26. H3BO3
27. CuCO3
28. LiH2PO3
29. Si3N4
30. MgSiO3
(6)
(7)
(8)
Name: _____________________
Period: ___
The Mole
(1) Find the molar mass of the following elements/compounds:
(a) W
(b) oxygen
(c) TiCl4
(d) sodium phosphate
(e) lead (II) sulphate
(2) Complete the following mole conversions:
(a) 1.80 mol Fe = ____________ g Fe
(b) 0.225 mol argon = ____________ atoms argon
(c) 8.9x1022 molecules CH4 = ____________ mol CH4
(d) 1.15 g CaO = ____________ mol CaO
(e) 84.2 g N2O = ____________ molecules N2O
(f) 2.54x1023 molecules NH3 = ____________ g NH3
(3) What is the mass of 6.84x1024 molecules of sulphur hexafluoride? What is the mass in kg?
(4) How many molecules are there in 0.320 kg magnesium chlorate? How many atoms are there of each element? How many
atoms are there in total?
(5) Find the percent composition of each element in the following compounds.
(b) lead (II) nitrate
(c) Sr3(PO4)2
(a) FeCl3
(6) Acetaminophen is the pain reliever found in Tylenol™. Acetaminophen has the formula C8H9NO2. Determine the percent
composition of each element.
(7) Epsom salt has a variety of medical and agricultural uses. Epsom salt has the chemical formula MgSO4 · 7H2O (magnesium
sulphate heptahydrate).
(a) Determine the percent composition of each element.
(b) Determine the percent composition of water.
(8) Determine the empirical formula of each the following compounds. Name each compound.
(a) 48.83% I and 51.17% F
(b) 69.94% Fe and 30.06% O
(c) 32.37% Na, 22.57% S, and 45.06% O
(9) Malonic acid is used in the manufacture of sleeping pills. A 5.500 g sample of malonic acid contains 1.904 g of carbon,
0.2131 g of hydrogen and the remainder is oxygen. Determine the empirical formula for malonic acid.
(10) Adipic acid, a compound used in the production of nylon, contains 49.31% carbon, 6.90% hydrogen, and 43.79% oxygen .
The molecular weight of adipic acid is 146.145 g/mol. Determine the molecular formula.
(11) Cyclohexane is common solvent for organic reactions. A 2.000 g sample contains 1.7126 g of carbon and 0.2874 g of
hydrogen. The molecular weight of cyclohexane is 84.1608 g/mol. Determine the molecular formula.
Answers:
(1) (a) 183.85 g/mol (b) 32.00 g/mol (c) 189.712 g/mol (d) 163.944 g/mol (e) 303.26 g/mol
(2) (a) 101 g Fe (b) 1.35x1023 atoms Ar (c) 0.15 mol CH4 (d) 0.0205 mol CaO (e) 1.15x1024 molecules N2O (f) 7.19 g NH3
(3) 1.66x103 g 1.66 kg
(4) 1.01x1024 molecules Mg(ClO3)2, 1.01x1024 atoms Mg, 2.02x1024 atoms Cl, 6.06x1024 atoms O, and 9.09x1024 atoms total
(5) (a) 34.4% Fe 65.6% Cl (b) 62.6% Pb 8.5% N 29.0% O (c) 58.1% Sr 13.7% P 28.3% O
(6) 63.5% C 6.0% H 9.3% N 21.2% O
(7) (a) 9.9% Mg 13.3% S 71.4% O 5.7% H (b) 51.2% H2O
(8) (a) IF7 iodine heptafluoride (b) Fe2O3 iron (III) oxide (c) Na2SO4 sodium sulphate
(9) C3H4O4
(10) C6H10O4
(11) C6H12
Name: _____________________
Period: ___
Chemical Reactions
(1) Balance the following chemical equations:
(a) H2 +
N2 → NH3
(g) NH3 +
(b) Al + HCl → AlCl3 +
(c) XeF4 +
(d) BF3 +
(e)
PCl5 +
B2O3 +
HF
AsF3 → PF5 + AsCl3
(f) Al + Cr2O3 → Al2O3 +
(i) MgNH4PO4 →
(j) NaOH +
(k) KCl + HNO3 +
(2) Classify each reaction. Complete and balance the chemical equation.
_______________ (a) Na + N2 →
_______________ (b) Al + CuCl2 →
_______________ (c) C3H8 +
O2 →
_______________ (d) HCl + KOH →
_______________ (e) HI →
_______________ (f) Li + Br2 →
_______________ (g) LiCl + AgNO3 →
_______________ (h) CaO +
Cl2 →
_______________ (i) K2O →
_______________ (j) Na + Al2(SO4)3 →
_______________ (k) SrBr2 + Li2CO3 →
_______________ (l) H2SO4 +
_______________ (m)
NaOH →
Mg(NO3)2 +
_______________ (n) Na + O2 →
_______________ (o) NCl3 →
_______________ (p)
C2H6 +
O2 →
Na3PO4 →
Mg2P2O7 +
NH3 +
H2O
Al2O3 + HF → Na3AlF6 +
(l) Ca3(PO4)2 +
Cr
H2O
H2O → NaBO2 + H2
(h) NaBH4 +
H2
H2O → Xe + O2 + HF
H2O →
O2 → NO +
O2 → KNO3 +
SiO2 +
C→
H2O
Cl2 +
CaSiO3 +
H2O
P4 + CO
(3) Complete and balance the following chemical equations:
(a)
MgCO3 →
(f)
(b) (NH4)2CO3 →
(c)
MgO +
SO3 →
(g) Ca(ClO3)2 →
CaO + H2O →
(h) NH4OH →
(d)
K2O +
CO2 →
(i) H2SO3 →
(e)
SO2 + H2O →
(j) H2CO3 →
Stoichiometry
(1) Silver is reacted with copper (II) chloride to produce silver chloride and copper. If 145 g of silver are present in the reaction,
what mass of copper (II) chloride is reaquired? What would be the mass of each of the products?
(2) Calcium chloride reacts with sodium sulphate to produce calcium sulphate and sodium chloride.
(a) If 5.5 g of sodium sulphate react, determine the mass of calcium chloride required.
(b) If 3.4 g of sodium chloride are actually produced, determine the percent yield of the reaction. What mass of calcium
sulphate will actually be obtained?
(3) Magnesium is reacted with oxygen to produce magnesium oxide.
(a) If 50.0 g of magnesium are reacted with 35.0 g oxygen, which reactant is limiting and which is excess?
(b) What is the mass of the product?
(c) What mass of the excess reactant is used in the reaction, and what mass of the excess reactant remains after the reaction?
(4) Aluminum chloride is reacted with silver nitrate to produce aluminum nitrate and silver chloride.
(a) If 30.6 g of aluminum chloride is reacted with 90.5 g of silver nitrate, which reactant is limiting and which is excess?
(b) What mass of the excess reactant is used in the reaction, and what mass of the excess reactant remains after the reaction?
(c) What is the actual mass of the products if the reaction has a percent yield of 75.0%?
Answers:
Chemical Reactions
(1) (a) 3H2 + N2 → 2NH3
(b) 2Al + 6HCl → 2AlCl3 + 3H2
(c) XeF4 + 2H2O → Xe + O2 + 4HF
(d) 2BF3 + 3H2O → B2O3 + 6HF
(e) 3PCl5 + 5AsF3 → 3PF5 + 5AsCl3
(f) 2Al + Cr2O3 → Al2O3 + 2Cr
(g) 4NH3 + 5O2 → 4NO + 6H2O
(h) NaBH4 + 2H2O → NaBO2 + 4H2
(i) 2MgNH4PO4 → Mg2P2O7 + 2NH3 + H2O
(j) 6NaOH + Al2O3 + 12HF → 2Na3AlF6 + 9H2O
(k) 4KCl + 4HNO3 + O2 → 4KNO3 + 2Cl2 + 2H2O
(l) 2Ca3(PO4)2 + 6SiO2 + 10C → 6CaSiO3 + P4 + 10CO
(2)
synthesis (a) 6Na + N2 → 2Na3N
combustion (c) C3H8 + 5O2 → 3CO2 + 4H2O
decomposition (e) 2HI → H2 + I2
double replacement (g) LiCl + AgNO3 → LiNO3 + AgCl
decomposition (i) 2K2O → 4K + O2
double replacement (k) SrBr2 + Li2CO3 → SrCO3 + 2LiBr
double replacement (m) 3Mg(NO3)2 + 2Na3PO4 → Mg3(PO4)2 + 6NaNO3
decomposition (o) 2NCl3 → N2 + 3Cl2
single replacement (b) 2Al + 3CuCl2 → 2AlCl3 + 3Cu
neutralization (d) HCl + KOH → KCl + H2O
synthesis (f) 2Li + Br2 → 2LiBr
single replacement (h) 2CaO + 2Cl2 → 2CaCl2 + O2
single replacement (j) 6Na + Al2(SO4)3 → 3Na2SO4 + 2Al
neutralization (l) H2SO4 + 2NaOH → Na2SO4 + 2H2O
synthesis (n) 4Na + O2 → 2Na2O
combustion (p) 2C2H6 + 7O2 → 4CO2 + 6H2O
(3)
(a) MgCO3 → MgO + CO2
(b) (NH4)2CO3 → 2NH3 +H2O + CO2
(c) CaO + H2O → Ca(OH)2
(d) K2O + CO2 → K2CO3
(e) SO2 + H2O → H2SO3
(f) MgO + SO3 → SO2 + H2O
(g) Ca(ClO3)2 → CaCl2 + 3O2
(h) NH4OH → NH3 + H2O
(i) H2SO3 → SO2 + H2O
(j) H2CO3 → CO2 + H2O
Stoichiometry
(1) 193 g AgCl 42.7 g Cu
(2) (a) 4.3 g CaCl2 (b) 75.6% 4.0 g CaSO4
(3) (a) lim: Mg ex: O2 (b) 82.9 g MgO (c) O2 used: 32.9 g mass O2 remaining: 2.1 g
(4) (a) lim: AgNO3 ex: AlCl3 (b) AlCl3 used: 23.7 g AlCl3 remaining: 6.9 g (c) 28.4 g Al(NO3)3 57.2 g AgCl
Name: _____________________
Period: ___
Solutions
(1) A solution contains 0.140 mol of sodium chloride in 2.80 L. Determine the concentration.
(2) A 0.200 M solution contains 26.6 g of aluminum chloride. Determine the volume.
(3) 525 mL of 0.20 M solution is diluted to a final volume of 850 mL. Determine the final concentration.
(4) What volume of water must be added to 1.80 L of 0.150 M solution to give a final concentration of 0.100 M?
(5) Write a dissociation equation for each compound. Determine the concentration of each ion.
(b) 8.0x10-3 M Na2CO3
(c) 0.020 M Al2(SO4)3
(a) 0.15 M AlCl3
(6) Classify the following compounds as soluble or insoluble in water.
(c) Sr(OH)2 (d) Fe(NO3)2
(e) CaS
(a) AgCl
(b) BaSO4
(i) Cs3PO4
(j) ZnCrO4
(k) CuI2
(l) Cd(OH)2
(m) Al2(SO4)3
(f) PbBr2
(g) BaF2
(h) MgCO3
(n) ScF3
(o) NiPO4
(p) HgS
(7) Write the net ionic equation for the each of following reactions. Give the spectator ions.
(a) LiI + AgNO3
(b) Na2CO3 + CaCl2
(c) (NH4)2S + Pb(NO3)2
(d) lead (II) nitrate + sodium sulphate
(e) lithium phosphate + zinc bromide
(f) sodium hydroxide + aluminum bromide
(8) Aluminum bromide solution is reacted with silver nitrate solution.
(a) What volume of 0.35 M aluminum bromide solution reacts with 150 mL of 0.25 M silver nitrate solution?
(b) What is the mass of each of the products?
(c) What is the net ionic equation for this reaction?
(9) 150 mL of 0.80 M lead (II) nitrate is reacted with 250 mL of 0.60 M sodium chloride.
(a) Which reactant is limiting and which is in excess?
(b) What is the mass of each of the products?
(c) What is the net ionic equation for this reaction?
Answers:
(1) 0.0500 M (2) 0.997 L (3) 0.12 M (4) 0.90 L added
(5) (a) AlCl3 → Al3+ + 3Cl- [Al3+] = 0.15 M [Cl-] = 0.45 M
(b) Na2CO3 → 2Na+ + CO32- [Na+] = 1.6x10-2 M [CO32-] = 8.0x10-3 M
(c) Al2(SO4)3 → 2Al3+ + 3SO42- [Al3+] = 0.040 M [SO42-] = 0.060 M
(6) (a) in (b) in (c) s (d) s (e) s (f) in (g) in (h) in (i) s (j) in (k) s (l) in (m) s (n) s (o) in (p) in
(7) (a) Ag+ (aq) + I- (aq) → AgI (s) spec ions: Li+ NO3(b) Ca2+ (aq) + CO32- (aq) → CaCO3 (s) spec ions: Na+ Cl(c) Pb2+ (aq) + S2- (aq) → PbS (s) spec ions: NH4+ NO3(d) Pb2+ (aq) + SO42- (aq) → PbSO4 (s) spec ions: Na+ NO3(e) 3Zn2+ (aq) + 2PO43- (aq) → Zn3(PO4)2 (s) spec ions: Li+ Br(f) Al3+ (aq) + 3OH- (aq) → Al(OH)3 (s) spec ions: Na+ Br(8) (a) 0.036 L (b) 2.7 g Al(NO3)3 7.0 g AgBr (c) Ag+ (aq) + Br- (aq) → AgBr (s)
(9) (a) lim: NaCl ex: Pb(NO3)2 (b) 21 g PbCl2 13 g NaNO3 (d) Pb2+ (aq) + 2Cl- (aq) → PbCl2 (s)
Name: _____________________
Period: ___
Gases
(1) Complete the following pressure conversions.
(a) 0.825 atm = _______ mm Hg = _______ kPa
(b) _______ atm = 850 mm Hg = _______ kPa
(2) A sample of 1.5 L of neon at 0.85 atm of pressure is expanded to 4.5 L. What will the resulting pressure be if the temperature
remains constant?
(3) A balloon contains 3.50 L of air at 30 °C. What will the volume of the balloon be if the temperature is lowered to 12 °C, if
the pressure remains constant?
(4) A gas cylinder has a pressure reading of 4.50x105 Pa at 305 K. At what temperature will the pressure read 8.50x105 Pa, if the
volume remains constant?
(5) A sample of oxygen occupies 105 mL at 305 K and 2.40 atm of pressure. What volume will the sample occupy at 345 K and
1.80 atm of pressure?
(6) What is the mass of 625 mL of argon gas at STP? How many atoms of argon are contained within this volume?
(7) What is the volume occupied by 3.02 mol of xenon at 0.950 atm and 385 K?
(8) What is the volume occupied by 20.5 g of water vapour at 9.80x104 Pa and 60 °C.
(9) Propane (C3H8) is combusted with oxygen to produce carbon dioxide and water vapour at STP. If 440 mL of propane react,
what volume and mass of oxygen is required? What is the volume and mass of each of the products?
(10) Nitrogen gas reacts with chlorine gas to produce nitrogen trichloride.
(a) If 250 L of nitrogen react with 450 L of chlorine at 180 kPa and 600 °C, which reactant is limiting and which is in excess?
(b) What volume and mass of nitrogen trichloride will be produced?
(11) Write the net ionic equation for each of the following reactions.
(a) K2S (aq) + HBr (aq) →
(g) Na2S (aq) + HNO3 (aq) →
(b) Na2CO3 (aq) + HI (aq) →
(h) Cs2SO3 (aq) + HI (aq) →
(c) NH4Br (aq) + NaOH (aq) →
(i) K2CO3 (aq) + HCl (aq) →
(d) Li2SO3 (aq) + HCl (aq) →
(j) NH4F (aq) + LiOH (aq) →
Answers:
(1) (a) 627 mm Hg 83.6 kPa (b) 1.12 atm 113 kPa
(2) 0.27 atm
(3) 3.29 L
(4) 576 K
(5) 0.158 L
(6) 1.68x1022 atoms 1.11 g
(7) 100 L
(8) 32.1 L
(9) 2.20 L and 3.14 g O2 1.32 L and 2.59 g CO2 1.76 L and 1.42 g H2O
(10) (a) lim: Cl2 ex: N2 (b) 300 L and 896 g NCl3
(11)
(a) 2H+ (aq) + S2- (aq) → H2S (g)
(g) 2H+ (aq) + S2- (aq) → H2S (g)
+
2(b) 2H (aq) + CO3 (aq) → CO2 (g) + H2O (l)
(h) 2H+ (aq) + SO32- (aq) → SO2 (g) + H2O (l)
+
(c) NH4 (aq) + OH (aq) → NH3 (g) + H2O (l)
(i) 2H+ (aq) + CO32- (aq) → CO2 (g) + H2O (l)
+
2(d) 2H (aq) + SO3 (aq) → SO2 (g) + H2O (l)
(j) NH4+ (aq) + OH- (aq) → NH3 (g) + H2O (l)
Name: _____________________
Period: ___
Complex Stoichiometry
(1) Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas.
(a) Write a balanced chemical equation for this reaction.
(b) If 250 mL of 0.50 M hydrochloric acid is reacted, what mass of aluminum is required?
(c) What is the resulting concentration of Al3+ and Cl- ions? (Note: the volume of solution remains constant)
(d) If the reaction takes place at 25 ºC and 1.02 atm, what volume of hydrogen gas is produced?
(2) Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide.
(a) Write a balanced chemical equation for this reaction.
(b) If 5.00 g of iron (III) oxide are reacted with 1.50 L of carbon monoxide at 22 ºC and 1.10 atm, which reactant is limiting
and which reactant is in excess?
(c) If only 2.10 g of iron are produced, what is the percent yield for the reaction? What mass of carbon dioxide will actually be
obtained?
(3) Ammonia reacts with carbon dioxide and water to produce ammonium hydrogen carbonate according to the following
balanced chemical equation:
NH3 + CO2 + H2O → NH4HCO3
If 150 mL of 0.250 M ammonia solution is reacted with 1.25 L of carbon dioxide gas at 30 ºC and 105 kPa in the presence of
excess water, what mass of ammonium hydrogen carbonate is produced if the reaction has a percent yield of 85.0%?
Answers:
(1) (a) 2Al + 6HCl → 2AlCl3 + 3H2
(2) (a) Fe2O3 + 3CO → 2Fe + 3CO2
(3) 2.52 g
(b) 1.1 g Al
(c) [Al3+] = 0.17 M [Cl-] = 0.50 M (d) 1.5 L
(b) lim: CO ex: Fe2O3 (c) 82.7% 2.48 g CO2