Download Introductory Chemistry Test Review

Chem 1405 Fall 2016
Exam 2 Review Practice Problems
1. Provide the chemical formula for each of the following chemical compounds:
a. Iron(II) sulfate
b. Barium nitrate
c. Copper(II) oxide
d. Magnesium hydroxide
e. Potassium chlorate
f. Lead(II) acetate
g. Ammonium sulfide
h. Silver carbonate
2. Indicate the name of the cation and its charge for each of the following binary ionic compounds:
a. CrO2
b. NaBr
c. ZnS
d. V2O3
e. SrF2
f. CaO
g. MgCl2
3.
Indicate the name of the anion and its charge for each of the following binary ionic compounds:
a. FeBr3
b. Ca(OH)2
c. ZnS
d. VCl3
e. Na3N
f. K3PO4
g. Al2O3
4.
Identify the polyatomic anion and its charge for each of the following ionic compounds:
a. Ca(C2H3O2)2
b. AlPO4
c. CuSO4
d. AgNO3
e. NiCO3
f. K2SO3
g. Pb(OH)2
5.
For the following chemical formulas, write the systematic names of each chemical compound:
a. SnCl4
b. VF5
c. SiC
d. CsBr
e. Ba3(PO4)2
f. Co(NO3)2
g. MgCO3
h. Ag2SO4
i. CaS
6.
For the following chemical formulas, write the systematic names of each chemical compound:
a. SCl4
b. PF5
c. SiO2
d. SeBr2
e. CS2
f. N2O5
g. P2Cl4
h. IF3
i. AsCl3
7. For the following compound names, write the systematic chemical formulas of each chemical
compound:
a. Dinitrogen monoxide
b. Phosphorus pentachloride
c. Iodine pentafluoride
d. Carbon tetrachloride
e. Selenium dioxide
f. Phosphorus trifluoride
g. Iodine trichloride
h. Arsenic trichloride
i. Sulfur trioxide
j. Oxygen difluoride
8. For the following aqueous chemical compounds, predict whether each will be a strong electrolyte,
a weak electrolyte, or a nonelectrolyte.
a. CaCl2
b. CH4
c. HF
d. C2H4O2
e. CH2O
9. For the following chemical compounds, predict whether each will be soluble or insoluble in
aqueous solution.
a. Al(OH)3
b. Hg2Cl2
c. (NH4)2CO3
10. For the following aqueous chemical reactions, predict the possible products and identify any
products that will be insoluble.
a. CaCl2 + K2S
b. MgCl2 + Na3PO4
11. Write a complete and balanced equation for the dissociation of the following compounds when
dissolved in water.
a. Na2SO4
b. FeCl3
12. Write a complete and balanced molecular equation for each of the following:
a. The aqueous reaction of calcium iodide with mercury(II) acetate.
b. The aqueous reaction of potassium phosphate with aluminum chloride.
13. Write the net ionic equation for the following aqueous chemical reactions.
a. AgNO3 + KI
b. H2CO3 + ZnCl2
14. Classify each of the following balanced chemical reactions, based on the type of reaction.
a. LiOH(s) + H2SO4(aq)
2H2O(l) + Li2SO4(aq)
b. C8H18(l) + O2(g)
CO2(g) + H2O(g)
c. 2Fe(s) + 3H2SO4(aq)
Fe2(SO4)3(s) + 3H2(g)
d. NaCl(aq) + AgNO3(aq)
AgCl(s) + NaNO3(aq)
15. For the following balanced redox reactions, identify which species lost electrons and which species
gained electrons.
a. 2 H2(g) + O2(g)
2 H2O(g)
b. SCl2(g) + Cl2(g) + 4 NaF(s)
SF4(g) + 4 NaCl(s)
16. For the following balanced redox reactions, determine the number of electrons transferred and
identify the donor and acceptor of the transferred electrons.
a. 4 Fe(s) + 3 O2(g)
2 Fe2O3(s)
b. Sn4+(aq) + Ca(s)
Sn2+(aq) + Ca2+(aq)
17. Balance the following chemical reactions:
a. NaHCO3(s) + H2SO4(aq)
Na2SO4(aq) + CO2(g) + H2O(l)
b. C3H5O9N3(l)
CO2(g) + N2(g) + O2(g) + H2O(g)
18. Calculate the molar mass of the following compounds.
a. NO2
b. C6H4Cl2
19. Calculate the mass percent of nitrogen in ammonium sulfide.
20. Calculate the number of moles of zinc that will be present in a 62.5g sample of pure zinc.
21. Calculate the mass in grams for 0.128 moles of potassium nitrate.
22. How many grams of KBrO3 are needed to produce 42.4 grams of Br2 in the following reaction?
KBrO3(s) + 5KBr(s) + 6HNO3(aq)
6KNO3(aq) + 3Br2(aq) + 3H2O(l)
23. For the following reaction, what mass of water is needed to completely react with 20.0 g of
phosphorus trichloride?
PCl3(g) + 3H2O(l)
H3PO3(aq) + 3HCl(aq)
24. Which substance is the limiting reactant when 14.00 g of calcium oxide reacts with 10.00 g of
carbon to produce 16.00 g of calcium carbide and 7.00 g of carbon dioxide according to the
following balanced chemical equation?
CaO(s) + 3 C(s)
CaC2(s) + CO(g)
25. In the laboratory, potassium chlorate will decompose when heated to form potassium chloride
and oxygen gas according to the following equation. Calculate how much oxygen in grams is
produced when 35.0 grams of potassium chlorate decomposes.
2 KClO3(s)
2KCl(s) + 3 O2(g)
26. Find the percent yield of product if 1.50 g of sulfur trioxide is produced from 1.00 g of oxygen gas
and excess sulfur via the reaction:
2 S(s) + 3 O2(g)
2 SO3(g)
27. Dimethyl sulfoxide, (CH3)2SO, can be prepared by the reaction of oxygen with dimethyl sulfide,
(CH3)2S,
2(CH3)2S(g) + O2(g)
2(CH3)2SO(l)
If this process is 83% efficient, how many grams of dimethyl sulfoxide could be produced from
65.0 g of dimethyl sulfide and excess O2?
28. Hydrogen peroxide can decompose to water and oxygen by the following reaction:
2 H2O2(l) → 2 H2O(l) + O2(g)
ΔH = –196 kJ/mol
Calculate the value of q when 5.00 g of H2O2(l) decomposes at constant pressure.
29. How much heat is evolved (in kJ) when 5.00 g of aluminum is reacted with a stoichiometric
amount of Fe2O3?
2 Al(s) + Fe2O3(s) → 2 Fe(s) + Al2O3(s)
ΔH = -852 kJ
30. How much heat is absorbed when 50.00 g of carbon reacts in the presence of excess SO2(g) to
produce CS2(l) and CO(g) according to the following chemical equation?
5 C(s) + 2 SO2(g)
CS2(l) + 4 CO(g)
ΔH = +239.9 kJ