Name: ______________________ Class: _________________ Date: _________
ID: A
Final Prep #3 Ch. 10-12
Short Answer
Balance the following chemical equations.
1. C2 H6 (g) + O2 (g) → CO2 (g) + H2 O(g)
2. Al(s) + HCl(aq) → AlCl3 (aq) + H2 (g)
3. CoCO3 (s) → CoO(s) + CO2 (g)
Write a balanced equation for each of the following reactions, substituting symbols and formulas for
names. Include the state of each reactant and product. Then identify the reaction type for each. If
more than one reaction type applies, list all that apply.
4. When aluminum nitrate and sodium hydroxide solutions are mixed, solid aluminum hydroxide forms.
The other product is sodium nitrate.
5. When solid copper(II) oxide and hydrogen react, metallic copper and water form.
6. When chlorine gas is passed through a potassium bromide solution, bromine forms in a potassium
chloride solution.
Predict the products in each of the following reactions. If no reaction occurs, write NR. You may use
Figure 10-10 for the relative activities of common metals and halogens.
7. Rb(s) + CaCl2 (aq)
8. F2 (g) + NaI(aq)
9. Zn(s) + AgNO3 (aq)
To prevent corrosion and make paints adhere better, some aluminum products are treated with
chromium(III) phosphate before finishing. Chromium(III) phosphate (CrPO4 ) is commercially
produced by treating chromium metal with orthophosphoric acid (H3 PO4 ).
10. Balance the following equation for the reaction.
_____Cr(s) + _____H3 PO4 (aq) → _____H2 (g) + _____CrPO4 (s)
Sand (silicon dioxide) and coke (carbon) are combined to form silicon carbide (SiC), a compound used in
high-strength ceramic materials.
11. Balance the following equation for the reaction.
_____SiO2 (s) + _____ C(s) → _____SiC(s) + _____ CO(g)
1
Name: ______________________
ID: A
Problem
Identify and calculate the number of representative particles in each of the following quantities.
12. 0.151 mole of nitrogen oxide
13. 11.5 moles of potassium bromide
Calculate the number of moles of the substance that contains the following number of representative
particles.
14. 5.50 × 102 5 molecules of carbon monoxide
Determine the mass in grams of each of the following quantities.
15. 3.35 moles of calcium
Calculate the number of moles in each of the following samples.
16. 6.35 g lithium
17. 3.75 g calcium carbide (CaC2 )
How many atoms are in the following samples?
18. 1.24 g cobalt
Which quantity has the greatest mass?
19. 4.16 × 102 3 atoms of radium
20. 1.33 × 102 4 atoms of argon
What is the mass in grams of each of the following quantities?
21. 4.62 moles of magnesium bromide (MgBr2 )
Calculate the number of moles in each of the following samples.
22. 245 g aluminum nitrite (Al(NO2 )3 )
Determine the percent composition of each of the following compounds.
23. manganese oxide (MnO)
24. propanol (C3 H8 O)
2
Name: ______________________
ID: A
Determine the empirical formula for a 100.00-g sample of a compound having the following percent
composition.
25. 94.07% sulfur and 5.93% hydrogen
26. 80.68% mercury, 12.87% oxygen, and 6.45% sulfur
Limestone (CaCO3 ) is treated with hydrochloric acid and water to manufacture calcium chloride
hexahydrate. This compound is used to melt ice and snow on pavements and roads. The following
balanced chemical equation represents the reaction.
CaCO3 (s) + 2HCl(aq) + 5H2 O(l) →
CaCl2 ·6H2 O(s) + CO2 (g)
27. How many moles of calcium chloride hexahydrate will be produced from 4.00 mol calcium carbonate?
Sand (silicon dioxide) and coke (carbon) are combined to form silicon carbide (SiC), a compound used in
high-strength ceramic materials.
28. What mass of silicon carbide will be produced from the reaction of 352 g silicon dioxide?
29. If 1.00 g of carbon is reacted, what mass of carbon monoxide is released?
3
ID: A
Final Prep #3 Ch. 10-12
Answer Section
SHORT ANSWER
1. ANS:
2C2 H6 (g) + 7O2 (g) → 4CO2 (g) + 6H2 O(g)
PTS: 1
2. ANS:
2Al(s) + 6HCl(aq) → 2AlCl3 (aq) + 3H2 (g)
PTS: 1
3. ANS:
CoCO3 (s) → CoO(s) + CO2 (g)
PTS: 1
4. ANS:
Al(NO3 ) 3 (aq) + 3NaOH(aq) → Al(OH)3 (s) +3NaNO3 (aq)
double-replacement
PTS: 1
5. ANS:
CuO(s) + H2 (g) → Cu(s) + H2 O(l)
single-replacement
PTS: 1
6. ANS:
Cl2 (g) + 2KBr(aq) → Br2 (l) + 2KCl(aq)
single-replacement
PTS: 1
7. ANS:
RbCl(aq) + Ca(s)
PTS: 1
8. ANS:
NaF(aq) + I2 (s)
PTS: 1
9. ANS:
Ag(s) + Zn(NO3 ) 2 (aq)
PTS:
1
1
ID: A
10. ANS:
__2___Cr(s) + __2___H3 PO4 (aq) → __3___H2 (g) + __2___CrPO4 (s)
PTS: 1
11. ANS:
__1___SiO2 (s) + __2___ C(s) → __1___SiC(s) + __2___ CO(g)
PTS:
1
PROBLEM
12. ANS:
PTS: 1
13. ANS:
PTS: 1
14. ANS:
PTS: 1
15. ANS:
PTS: 1
16. ANS:
PTS:
1
2
ID: A
17. ANS:
PTS: 1
18. ANS:
PTS: 1
19. ANS:
PTS: 1
20. ANS:
PTS:
1
3
ID: A
21. ANS:
PTS: 1
22. ANS:
PTS:
1
4
ID: A
23. ANS:
PTS: 1
24. ANS:
PTS:
1
5
ID: A
25. ANS:
PTS: 1
26. ANS:
PTS: 1
27. ANS:
PTS:
1
6
ID: A
28. ANS:
PTS: 1
29. ANS:
PTS:
1
7