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9 Pages
Chem Exam I
Course: CHEM 1311, Spring 2008School: TAMU Corp. Chr.
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1311 CHEM / PRACTICE EXAM II / CHAPTERS 4 & 5 / 150 POINTS DATE: ________________ YOUR NAME: _______________________________ (please print) POINT TOTALS: I. Multiple-Choice ___/100 II. Problem-Solving ___/50 Sum = ____/150 Part I. Multiple Choice (100 Points Total) Directions: Circle the letter adjacent the one best response. You are not required to show your work for this portion of the exam. You may...
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1311 CHEM / PRACTICE EXAM II / CHAPTERS 4 & 5 / 150 POINTS DATE: ________________ YOUR NAME: _______________________________
(please print)
POINT TOTALS: I. Multiple-Choice ___/100
II. Problem-Solving ___/50 Sum = ____/150
Part I. Multiple Choice (100 Points Total)
Directions: Circle the letter adjacent the one best response. You are not required to show your work for this portion of the exam. You may write next to the problem, but I will only grade your circled answer. If you circle more than one response per question then you will lose all credit for that problem.
#01. (5 pts) To which category does the following reaction belong? PbSO4(aq) + K2O(s) PbO(s) + K2SO4(aq) a. a gas-forming reaction b. an acid-base reaction c. a precipitation reaction d. an oxidation-reduction reaction e. none of the above #02. (5 pts) Determine the oxidation number of chromium in H 2CrO4. You may want to may use of the oxidation number table on page 8. a. Cr+ b. Cr2+ c. Cr3+ d. Cr4+ e. Cr6+ #03. (5 pts) Which one of the following is a weak acid? a. HCl b. HNO3 c. H2SO4 d. HBr e. Acetic acid (C2H4O2) #04. (5 pts) Oxidation-reduction reactions always involve ____________ . a. the transfer of electrons b. an oxidizing agent c. a reducing agent d. a precipitate e. a, b & c
CHEM 1311/TAMUCC/J. M. Southard, PhD
1
#05. (5 pts) Balance the acid-base reaction with the smallest whole number coefficients. I've placed blanks in front of each compound for your convenience. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one". __ Ca(OH)2 + __ H3PO4(aq) __ Ca3(PO4)2(aq) a. 4 b. 5 c. 8 d. 9 e. 12 #06. (5 pts) Based on the following balanced equation determine how many moles of O 2 are required to react with 23.5 moles of CH3OH? 2 CH3OH(l) + 3 O2(g) 2 CO2(g) + 4 H2O(g) a. 47.0 b. 35.3 c. 11.8 d. 40.0 e. 23.5 #07. (5 pts) Based on the following balanced equation determine how many moles of H2 can be produced from 72.9 g Mg and an excess of HCl. 2 HCl(g) + Mg(s) MgCl2(s) + H2(g) a. 4.50 mol b. 3.00 mol c. 1.50 mol d. 9.00 mol e. 6.00 mol #08. (5 pts) What is the identity of the "oxidizing agent" in the following oxidation-reduction reaction? 2 Mg(s) + S2(g) 2 MgS(s) a. Mg b. S2 c. MgS d. This reaction does not involve electron-transfer e. None of the above
CHEM 1311/TAMUCC/J. M. Southard, PhD
+
__ H2O(l)
2
#09. (5 pts) Based on the following balanced equation, what mass of SiF 4 could be produced by the reaction of 15.0 g SiO2 with an excess of HF? SiO2(s)
FW 60.08
+
4 HF(l)
FW 20.01
SiF4(l)
FW 104.08
+ 2 H2O(l)
FW 18.02
a. 1.04 g b. 12.0 g c. 26.0 g d. 104 g e. 52.0 g
#10. (5 pts) What is the net ionic equation for the following formula unit equation? Cu(NO3)2(aq) + Na2CO3(aq) CuCO3(s) + 2 NaNO3(aq) a. Cu2+(aq) + CO32-(aq) CuCO3(s) b. Cu2+(aq) + 2 NO3-(aq) + 2 Na+(aq) + CO32-(aq) CuCO3(s) + 2 Na+(aq) + 2 NO3-(aq) c. Cu2+(aq) + 2 NO3-(aq) + 2 Na+(aq) CuCO3(s) + 2 Na+(aq) + 2 NO3-(aq) d. Cu2+(aq) + CO32-(aq) Cu2+(s) + CO32-(s) e. 2 NO3-(aq) + 2 Na+(aq) 2 NaNO3(s) #11. (5 pts) Based upon the following balanced equation, how many grams of HNO 3 can be prepared from the reaction of 69.0 grams of NO 2 with 36.0 grams of H2O? 3 NO2(g) +
FW 46.01
H2O(l)
FW 18.02
2 HNO3(aq) +
FW 63.01
NO(g)
FW 30.01
a. 252 g b. 63.0 g c. 116 g d. 84.0 g e. 76.0 g
CHEM 1311/TAMUCC/J. M. Southard, PhD
3
#12. (5 pts) What is the percent yield of elemental sulfur (S) if 7.54 grams of sulfur are obtained from the reaction of 6.16 grams of SO 2 with an excess of H2S? 2 H2S(g) +
FW 34.08
SO2(g)
FW 64.06
2 H2O(l) +
FW 18.02
3 S(s)
FW 32.07
a. 72.6% b. 40.8% c. 81.5% d. 88.4% e. 91.4% #13. (5 pts) You produce aspirin in lab. Theoretically, you determine that 6.25 grams aspirin may be produced. However, after you isolate your aspirin you determine that made 4.82 grams of aspirin. What is the percent yield for your efforts? a. 77.1% b. 22.9% c. 29.7% d. 130% e. 53.9% #14. (5 pts) Complete the reaction by balancing and indicating the phases (or states) on the product-side. You may need to make use of the solubility-table (on page 8). Na2CO3(aq) + CuCl2(aq) a. 2 NaCl(aq) + CuCO3(s) b. 2 NaCl(aq) + CuO(s) + CO2(g) c. 2 NaCl(s) + CuCO3(aq) d. 2 Na(s) + Cl2(g) + e. CuCO3(s) Na2Cu(s) + Cl2O2(g) + CO(g) #15. (5 pts) Which of the following is an example of a weak base? a. HCl b. CO2 c. H2SO4 d. NH3 e. All of these are weak bases
CHEM 1311/TAMUCC/J. M. Southard, PhD
+
4
#16. (5 pts) Which of the following substance(s) is/are insoluble in water? You may want to make use of the solubility-table (on page 8). a. NaBr b. PbBr2 c. AgCl d. NH4NO3 e. Both b and c
#17. (5 pts) Complete the reaction by balancing and indicating the phases (or states) on the product-side. Na2CO3(aq) + 2 HCl(aq) a. 2 NaCl(aq) + H2CO3(aq) b. 2 NaCl(aq) + H2O(l) + CO2(g) c. 2 NaCl(s) + H2CO3(aq) d. 2 Na(s) + Cl2(g) + H2O(l) + CO2(g) e. NaHCO3(aq) + NaCl(aq) + HCl(aq) +
#18. (5 pts) What volume, in milliliters, of 0.125 M NaOH would be needed to neutralize 25.0 mL of 0.234 M HCl? Equation: CaVa = CbVb. a. 13.4 mL b. 3.13 mL c. 5.85 mL d. 46.8 mL e. 25.0 mL
#19. (5 pts) What is the molarity of a solution made by dissolving 57.6 g of sodium iodide (NaI, FW = 149.89) in sufficient H2O to produce a total volume of 1.00 L? a. 8.63 M b. 0.384 M c. 2.60 M d. 8.63 103 M e. 0.116 M
CHEM 1311/TAMUCC/J. M. Southard, PhD
5
#20. (5 pts) Determine the oxidation number of carbon in H2CO3. You may want to may use of the oxidation number table on page 8. a. C+ b. C2+ c. C3+ d. C4+ e. C6+ Part II. Problem Solving (50 Points Total)
Read this! Directions: Please represent your work neatly. Remember the "setup" for each problem you solve is more important than the final answer. You must show your work for credit. For problems involving calculations please express final answers with the appropriate number of significant digits.
#21. (10 pts) What is the maximum mass of Ni(OH) 2 that could be prepared by mixing two solutions that contain 25.9 g NiCl 2 and 10.0 g NaOH, respectively? This is a limiting reagent type problem. For full credit you must show your work and express your answer with the appropriate number of significant digits. NiCl2(aq) + 2 NaOH (aq) Ni(OH)2(s) + 2 NaCl(aq)
FW 129.60 FW 40.00 FW 92.71 FW 58.44
#22. (10 pts) Provide (a) the total ionic equation and (b) the net ionic equation for the following balanced precipitation reaction. CdCl2(aq) + 2 NaOH(aq) Cd(OH)2(s) + 2 NaCl(aq)
CHEM 1311/TAMUCC/J. M. Southard, PhD
6
#23. (10 pts) Sulfur dioxide, a pollutant produced by burning coal and oil in power plants, can be removed by reaction with calcium carbonate: 2 SO2(g) + 2 CaCO3(s) +
FW 64.06 FW 100.09
O2(g)
FW 32.00
2 CaSO4(s) + 2 CO2(g)
FW 136.14 FW 44.01
(a) What mass of CaCO3 is required to remove 155 g of SO2? (b) What mass of CaSO4 is formed when 155 g of SO2 is consumed completely?
#24. (2 5 pts) (a) What is the pH of a 0.0145 M HCl solution? (b) What is the H+ concentration of a solution that has a pH = 1.36? Equations: pH = -log[H+] & [H+] = 10-pH.
#25. (10 pts) If 38.55 mL of HCl is required to titrate 2.150 g Na 2CO3 according to the following equation, what is the molarity of the HCl solution? Na2CO3(aq) + 2 HCl(aq) 2 NaCl(aq) + CO2(g) + H2O(l)
FW 106.00
CHEM 1311/TAMUCC/J. M. Southard, PhD
7
Solubility Table Soluble Compounds Almost all salts of Na+, K+, NH4+ Salts of NO3-, ClO3-, ClO4-, CH3CO2Exceptions Almost all salts of Cl , Br , I Compounds containing FSalts of sulfate, SO42Insoluble Compounds Most salts of CO32-, PO43-, C2O42-, CrO42Most metal sulfides, S2Most metal hydroxides & oxides Ba(OH)2 is moderately soluble
-
Halides of Ag , Hg22+, Pb2+ Fluorides of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ Sulfates of Ca2+, Sr2+, Ba2+, Pb2+ Exceptions Salts of NH4+ & alkali metal cations
+
Oxidation Numbers 1. Each atom in a pure element has an oxidation number of zero 2. For monatomic ions, the oxidation number is equal to the charge on the ion 3. Fluorine always has an oxidation number of -1 in compounds with all other elements 4. Cl-, Br-, I-, always have oxidation numbers of -1 in compounds except when combined with oxygen or fluorine 5. The oxidation number of H is +1 and O is -2 in compounds/ions Exceptions: a. H is -1 in binary compounds with metals b. O is -1 in peroxides 6. The algebraic sum of oxidation numbers for the atoms in a neutral sum compound must be zero; in a polyatomic ion the sum must be equal to the ion
CHEM 1311/TAMUCC/J. M. Southard, PhD
8
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