Department of Chemistry, Geosciences, and Environmental Science
Chemistry 1054-010 College Chemistry Fall 2009
(Please write your name legibly)
Read all directions and questions carefully!! This exam consists of two parts. The first part consists of 10 multiple choice questions worth four points each for a total of 40 points. The second part consists of five numerical problems worth either 10 or 15 points per question for a total of 60 points. Show all your work necessary for the numerical problems as partial credit will be given for those problems.
Possibly Useful Constants
Avogadro’s Number: NA = 6.022 × 1023 particles/mol
q = (heat capacity)×∆T
q = (mass in grams)×(specific heat)×∆T
q = (number of moles)×(molar heat capacity)×∆T
Calorimetry: qrxn = –Ccalorimeter×∆T or
qrxn = –(mass of solution)×(specific heat of solution)×∆T
Part 1 (40 points):_____________________
Part 2 (60 points):_____________________
Total (100 points):_____________________
Don’t forget to put your name on this test!
Please indicate the answer to each question by putting your choice in the space provided. There is only one correct answer for each question. There will be 10 multiple choice questions worth 4 points each.
1. Which of the following compounds is not a strong electrolyte.
(a) CCl4 (c) HCl
(b) NaCl (d) MgCl2
(e) All of the above are strong electrolytes
Answer: A (CCl4 contains only nonmetal atoms so it is a nonelectrolyte)
2. Which of the following are strong acids?
(a) HF and HBr (c) HI, HNO3, and HBr
(b) HI, HNO3, HF, and HBr (d) HNO3, HF, HBr
(e) HI, HF, and HBr
3. There are __________ mol of potassium ions in 0.500 L of a 0.300 M solution of K3PO4?
(a) 0.0500 (c) 0.150
(b) 0.167 (d) 0.500
Answer: E (= 0.500 L × 0.300 M × 3 mol K+)
4. In which species does sulfur have the highest oxidation number?
(a) S8 (c) H2S
(b) SO2 (d) SO32-
5. Oxidation cannot occur without ___________________.
(a) acid (c) water
(b) oxygen (d) reduction
6. The DE of a system that releases 12.4 J of heat and does 4.2 J of work on the surroundings is _________ J.
(a) 16.6 (c) 4.2
(b) 12.4 (d) –8.2
Answer: E (= –12.4 J + –4.2 J)
7. The value of DH° for the following reaction is –3351 kJ:
2 Al(s) + 3 O2(g) ¾¾® 2 Al2O3(s)
The value of DHf° for Al2O3(s) is ______________ kJ.
(a) –3351 (c) –2.86
(b) –1676 (d) –16.43
Answer: B This equation is double the formation reaction for Al2O3
8. A _____________ DH corresponds to an _______________ process.
(a) negative, endothermic (c) positive, exothermic
(b) zero, exothermic (d) negative, exothermic
(e) zero, endothermic
9. Which of the following is not considered a fossil fuel?
(a) coal (c) natural gas
(b) petroleum (d) hydrogen gas
(e) crude oil
10. When solutions of CaCl2 and Na2CO3 are mixed, a precipitate of CaCO3 is formed according to the reaction: CaCl2(aq) + Na2CO3(aq) ¾¾® CaCO3(s) + 2 NaCl(aq)
What are the spectator ions in this reaction?
(a) Ca2+ only (c) Na+ only
(b) Na+ and Cl¯ (d) Ca2+ and CO32-
(e) Cl¯ and CO32-
Solve the following problems, keeping track of significant figures where applicable. Please show all the work necessary to obtain your answer in order to receive partial credit for possibly wrong answers. Generally, full credit will not be given for the correct answer without any of the work performed to obtain the answer being shown on the paper. Each question is worth either 10 or 15 points.
11. (10 points) Calculate the volume in milliliters of 1.25 M (NH4)2SO4 solution that contains 35 g of (NH4)2SO4.
Calculate moles of (NH4)2SO4:
Calculate volume of solution in L:
Convert to mL:
12. (15 points) What is the molarity of a H2SO4 solution if it requires 26.36 mL of the H2SO4 solution to neutralize 58.46 mL of 0.1376 M NaOH? The acid-base neutralization reaction is:
H2SO4(aq) + 2 NaOH(aq) ¾¾® Na2SO4(aq) + 2 H2O(l)
Known: 58.46 mL of 0.1376 M NaOH
Unknown: 26.36 mL of ?? M H2SO4
Calculate moles of NaOH:
Convert to moles of H2SO4:
Calculate molarity of H2SO4:
13. (10 points) Calculate DH° for the following reaction given the table of thermodynamic data on the back of this exam:
2 NO2(g) + 7 H2(g) ¾¾® 2 NH3(g) + 4 H2O(g)
Getting the data from Appendix C in your book:
14. (10 points) Write the net ionic equation for each of the following reactions:
(a) 2 HI(aq) + Ba(OH)2(aq) ¾¾® BaI2(aq) + 2 H2O(l)
Total ionic equation:
2 H+(aq) + 2 I¯(aq) + Ba2+(aq) + 2 OH¯(aq) ¾¾® Ba2+(aq) + 2 I¯(aq) + 2 H2O(l)
Removing the spectator ions Ba2+ and I¯, the net ionic equation is:
2 H+(aq) + 2 OH¯(aq) ¾¾® 2 H2O(l)
(b) Ca(NO3)2(aq) + Na2CO3(aq) ¾¾® CaCO3(s) + 2 NaNO3(aq)
Total ionic equation:
Ca2+(aq) + 2 NO3¯(aq) + 2 Na2+(aq) + CO32-(aq) ¾¾® CaCO3(s) + 2 Na+(aq) + 2 NO3¯(aq)
Removing the spectator ions Na+ and NO3¯, the net ionic equation is:
Ca2+(aq) + CO32-(aq) ¾¾® CaCO3(s)
(c) Zn(s) + Sn(NO3)2(aq) ¾¾® Zn(NO3)2(aq) + Sn(s)
Total ionic equation:
Zn(s) + Sn2+(aq) + 2 NO3¯(aq) ¾¾® Zn2+(aq) + 2 NO3¯(aq) + Sn(s)
Removing the spectator ion NO3¯, the net ionic equation is:
Zn(s) + Sn2+(aq) ¾¾® Zn2+(aq) + Sn(s)
15. (15 points) When 50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NH3 in a coffee cup calorimeter, the temperature of the solution upon mixing increases from 21.2°C to 26.4°C. Assuming that the density of the solution is equal to 1.00 g/mL and that the heat capacity of the solution is 4.18 J/g·°C, calculate the heat of this reaction and the heat of reaction per mole of HCl.
50.0 mL of 0.10 M HCl mixed with 50.0 mL of 0.10 M NH3
Specific heat=4.18 J/g·°C
Density of solution=1.00 g/mL
Calorimetry problem: qrxn = –(mass of solution)(specific heat)DT
Calculate mass of solution:
Mass of solution = volume of solution ×density
=(50.0 mL+50.0 mL)×1.00 g/mL
Calculate heat of reaction:
qrxn = (100.0 g)(4.18 J/g·°C)(26.4°C–21.2°C) = (100.0 g)(4.18 J/g·°C)(5.2°C)
=–2200 J = –2.2 kJ
Calculate moles of HCl:
Moles of HCl = (50.0 mL/1000 mL/L)(0.10 M) = 0.0050 mol
Heat of reaction per mole:
(10 points extra credit) Give the complete definition for 2 out of the 3 terms below. 5 points will be given for each correct complete definition. Clearly note which 2 definitions you want graded, if you write three definitions without a clear notation, only the first two will be graded.
Oxidation: the loss of electrons by a substance
Specific heat: the amount of heat required to raise the temperature of one gram of an object by 1°C or 1 K.
Exothermic reaction: a reaction that gives off heat.