finala - Final Exam May 2 2008 CH101 Section 003 Dr T Brent...

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Final Exam May 2, 2008 CH101 Section 003 Dr. T. Brent Gunnoe Your Name: ______PINK Key ____________________________ INSTRUCTIONS 1) The answer sheet is double sided and is separate from the exam. BE CERTAIN TO PUT YOUR NAME ON THE ANSWER SHEET. When you are finished, turn in your exam and the answer sheet. THE ONLY ANSWERS THAT WILL COUNT ARE THOSE ON YOUR ANSWER SHEET. Your exam will not be returned, only the answer sheet. 2) You may use the back of each page for scrap paper. 3) Unless you indicate otherwise via an email to Prof. Gunnoe, your exam will be returned in class by placing in a folder with the first letter of your last name. 4) TURN OFF YOUR CELL PHONE! 5) When you complete the exam, quietly turn in all pages at the front of the room. Avogadro's number = 6.022 x 10 23 F = k q 1 q 2 /( ε r 2 ) E = kq 1 q 2 /( ε r ) c = νλ E = h ν ν = R H [(1/n lo 2 )-(1-n hi 2 )] R H = 3.29 x 10 15 Hz h = 6.6 x 10 -34 Js c = 3 x 10 8 m s -1 Δ Gº = - nF ε º Δ E system = q + w Δ H = sum(bonds broken) – sum(bonds formed) Δ S q/T Δ G = Δ H - T Δ S Δ Gº = -RT ln K eq Δ H solution = Δ H solute + Δ H solvent + Δ H mixing ε º cell = ε º cathode - ε º anode Solubility Rules 1) Compounds of NH 4 + and group 1A metals are soluble 2) Compounds of NO 3 - , ClO 4 - , ClO 3 - and C 2 H 3 O 2 - are soluble 3) Compounds of Cl - , Br - and I - are soluble except those of Ag + , Cu + , Tl + , Hg 2 2+ and Pb 2+ 4) Compounds of SO 4 2- are soluble except those of Ca 2+ , Sr 2+ , Ba 2+ and Pb 2+ 5) Most other ionic compounds are insoluble
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C 2 H 3 O 2 - acetate ion NH 4 + ammonium ion OH - hydroxide ion SO 4 2- sulfate ion SO 3 2- sulfite ion MnO 4 - permanganate ion CrO 4 2- chromate ion NO 3 - nitrate ion NO 2 - nitrite ion Bond Dissociation Energies (in kJ/mol) C-H 413 N-H 391 O-H 463 N-N 163 N=N 418 N N 941 C-F 485 N-F 272 O-F 190 H-H 436 C=O 799 C-O 358 C-C 347 C=C 612 C C 820 C-Cl 328 Cl-Cl 243 O=O 495 Table of Standard Reduction Potentials. Ox + ne 1- Red E o (V) K 1+ (aq) + e 1- K(s) -2.92 Na 1+ (aq) + e 1- Na(s) -2.71 Mg 2+ (aq) + 2e 1- Mg(s) -2.36 Al 3+ (aq) + 3e 1- Al(s) -1.66 2H 2 O + 2e 1- H 2 (g)+ 2OH 1- (aq) -0.83 Zn 2+ (aq) + 2e 1- Zn (s) -0.76 Cr 3+ (aq) + 3e 1- Cr(s) -0.74 Fe 2+ (aq) + 2e 1- Fe(s) -0.44 2H 2 O + 2e 1- H 2 (g)+ 2OH 1- (aq) -0.41 a PbSO 4 (s) + 2e 1- Pb(s) + SO 4 2- (aq) -0.36 Ni 2+ (aq) + 2e 1- Ni(s) -0.23 Sn 2+ (aq) + 2e 1- Sn(s) -0.14 Pb 2+ (aq)+ 2e 1- Pb(s) -0.13 2H 1+ (aq) + 2e 1- H 2 (g) 0.00 Cu 2+ (aq) + 2e 1- Cu(s) +0.34 O 2 (g) + 2H 2 O + 4e 1- 4OH 1- (aq) +0.40 I 2 (s) + 2e 1- 2I 1- (aq) +0.54 Fe 3+ (aq) + e 1- Fe 2+ (aq) +0.77 Ag 1+ (aq) + e 1- Ag(s) +0.80 O 2 (g) + 4H 1+ (aq) + 4e 1- 2H 2 O +0.82 a NO 3 1- (aq) + 4H 1+ (aq) + 3e 1- NO(g) +2H 2 O +0.96 Br 2 (l) + 2e 1- 2Br 1- (aq) +1.09 O 2 (g) + 4H 1+ (aq) + 4e 1- 2H 2 O +1.23 Cr 2 O 7 2- (aq) + 14H 1+ + 6e 1- 2Cr 3+ (aq) + 7H 2 O +1.33 Cl 2 (g) + 2e 1- 2Cl 1- (aq) +1.36 MnO 4 1- (aq) + 8H 1+ + 5e 1- Mn 2+ (aq) + 4H 2 O +1.51 PbO 2 (s) + 4H
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This note was uploaded on 05/21/2008 for the course CH 101 taught by Professor Bigham during the Spring '08 term at N.C. State.

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finala - Final Exam May 2 2008 CH101 Section 003 Dr T Brent...

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