Advanced Chemistry Semester II Review Problems
1. Aqueous potassium chromate and aqueous copper (II) chloride react in a double replacement reaction. Write and
balance the reaction showing symbols for solid, liquid, gas and aqueous.
2. Write net ionic equations for any precipitates resulting from mixtures of these aqueous solutions:
a) KI + (NH4)2CO3
b) Pb(NO3)2 + CaCl2
c) CaS + MgSO4
d) NaOH + HCl
3. Balance these equations:
a)
Li2O
+
H2O 
LiOH
b) Pb(C2H3O2)2
+
H2S 
PbS +
c)
C7H6O3
+
C4H6O3

C9H8O4
d)
CCl4
+
SbF3 
CCl2F2
+
HC2H3O2
+
H2O
SbCl3
4. Categorize each of the following reactions as single replacement (SR), double replacement (DR), synthesis (S),
decomposition (D) or combustion (C).
_____ a) Ca + O2  CaO
_____ b) Mg(NO3)2 + Cu  CuNO3 + Mg
_____ c) C4H10 + O2  CO2 + H2O
_____ d) Al2O3  Al + O2
_____ e) SrCl2 + F2  SrF2 + Cl2
_____ f) Ba(OH)2 + H3PO4  Ba3(PO4)2 + H2O
5.
a)
b)
c)
d)
e)
Write complete & balanced chemical equations for these reactions.
Synthesis reaction between oxygen and lithium
Decomposition of potassium bromide
Single replacement between phosphorus and nickel (II) sulfide
Double replacement between barium cyanide and hydrogen chloride
Combustion of C4H8OH
6. A compound was found to contain only carbon and hydrogen in a mass ratio of 6.0 g C to 1.0 g H. What is the
empirical formula of this compound?
7. A substance with a molar mass of 92 g consists of equal numbers of S and N atoms. What is the formula?
8. What is the percent of oxygen in calcium carbonate by mass?
9. Calculate the molar mass of ammonium dichromate.
10. What is the mass in grams of 7.213x1025 atoms of lead?
11. How many molecules are in 38.49 g of xenon hexafluoride?
12. Calculate the % composition of metal in zinc nitrate.
13. Determine the empirical formula for a compound containing 32.00% C, 42.66%O, 18.67% N and 6.67% H
14. What is the molecular formula for each of these compounds?
a) CH2O, molar mass = 90 g/mol
b) HgCl, molar mass = 472.2 g/mol
c) C3H5O2, molar mass = 146 g/mol
15. How many moles are in 401.2 mg of mercury?
16. How many moles of oxygen are needed to produce 9 moles of carbon dioxide in the combustion of C3H8?
17. What is the maximum mass of water that can be obtained by drying 2.0 moles of the hydrate sodium thiosulfate
pentahydrate?
18. A gas occupies a volume of 2.0 liters at 800 kPa and 45˚C. What volume does this gas occupy at 400 kPa and 258˚C?
19. You have three identical metal spheres. The first contains air (mostly nitrogen), the second contains helium at the
same temperature and pressure as the first and the third contains a vacuum (no atoms at all). Arrange these three systems
from most to least mass and EXPLAIN.
20. How many grams of potassium dichromate are needed to prepare 2.0 L of a 0.100 M solution?
21. What is the pH of 0.001 M hydrochloric acid?
22. What is the hydronium ion concentration of a solution in which the pH is 5.2?
23. You have 26.4 g of O2 in a container twice the size as one with CO2. The pressure and temperature are the same.
How many grams of CO2 do you have?
24. In a reaction, 24.9 L of gaseous nitrogen reacts with excess hydrogen gas to produce gaseous ammonia. How many
liters of ammonia were produced? This reaction does not occur at STP.
25. What mass of precipitate is obtained from 18.7 g of aluminum chloride and 18.7 g calcium hydroxide?
26. Aluminum metal reacts with zinc chloride in a single replacement reaction.
a) If 13.5g of Al reacts with 0.82 mol ZnCl2, which will be the limiting reagent?
b) If only 65.6g of aluminum chloride is produced, what is the percent yield?
27. What is the hydroxide ion concentration of a 0.27 M solution of hydrobromic acid?
28. A sample of carbon dioxide has a mass of 11.0 g at 273 K and 108.29 kPa. What is its volume?
29. Solid copper (I) sulfide reacts with oxygen gas forming solid copper (I) oxide and sulfur dioxide gas. How many
grams of copper (I) sulfide will react with 47.2 L of oxygen at STP.
30. In lab a student mixed 3.00 ml of 0.590 M sodium hydroxide with 5.00 ml of 1.27 M copper (II) nitrate. How many
grams of precipitate were formed?
31. In solution, the following reaction takes place: NH2- + NH4+  2 NH3. Identify any Bronsted acids, bases,
Arrhenius acids or bases present on the reactant side of the equation.
32. Consider a battery using a potassium electrode and a nickel electrode.
a) Identify the direction of electron flow.
c) What substance is the reducing agent?
b) Which metal is the anode?
d) Will the concentration of K+ ions increase or decrease?
33. In the unbalanced reaction, Fe + XO2  X + Fe2O3, list three metals the element X might be.
34. A gas sample expands from 3.00 to 5.00 liters at a constant pressure. If the initial temperature was -58˚C, what is the
final temperature?
35. How many grams of copper are replaced by 5.6 g of iron in this reaction? Fe(s) + CuCl2 (aq)  FeCl3(aq) + Cu (s)
36. 40.00 milliliters of 2.00 M potassium hydroxide reacts completely with 30.00 ml of nitric acid. What is the molarity
of the acid?
37. 6.9 grams of a gas occupies 2.24 liters at 273 K and 1 atm. The empirical formula is CH2. What is the molecular
formula?
38.
a)
b)
c)
Consider a battery made from Al, AlCl3, Fe and FeCl2 ions.
Which electrode is the cathode?
d) Which direction are electrons flowing?
Write the balanced half-reactions for each half-cell.
e) Which electrode will disintegrate over time?
Which substance is the oxidizing agent?
f) What is the electrode potential for this reaction?
39. Calculate cell potentials for these reactions & identify which ones are spontaneous reactions and which are not:
a) Na + Cl2  NaCl
b) SnCl4  SnCl2 + Cl2
c) HgI2  Hg + I2
40. What is the percent yield if 45 g of FeS2 produces 16 g of SO2 in the following reaction?
FeS2(s) + O2(g)  Fe2O3(s) + SO2(g)
41. Which of the following reactions will NOT take place? Why?
a) HOH + Na
b) Ag + CuNO3
c) F2 + CuCl2
d) Zn + HCl
e) Cl2 + KBr
42. For the above reactions that do occur, identify the element that is being reduced and the element that is being
oxidized, the oxidizing agent and the reducing agent and write balanced half-reactions for both.
43. If 75.0 mL of a iron (III) thiosulfate solution reacts with excess magnesium metal, producing 0.250 g of iron, what
was the molarity of the iron (III) thiosulfate solution?
44. What volume of hydrogen gas will evolve if 5.73 grams of zinc are mixed with 8.35 ml of 0.250 M hydrochloric acid
at STP?