SUPPL INSTR FOR CH 302 (GE 206E) - AnswersPPgalvaniccells2

SUPPL INSTR FOR CH 302 (GE 206E) - AnswersPPgalvaniccells2...

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Practice Problems: Galvanic Cells, part 2 1. Identify the reactions with K > 1 and for each such reaction identify the oxidizing agent and calculate the standard cell emf: (a) Cl 2 (g) + 2 Br - (aq) 2 Cl - (aq) + Br 2 (l) (b) MnO 4 - (aq) + 8H + (aq) + 5 Ce 3+ (aq) 5 Ce 4+ (aq) + Mn 2+ (aq) + 4 H 2 O(l) (c) 2 Pb 2+ (aq) Pb(s) + Pb 4+ (aq) 2. Find the unknown quantity: Pt(s) H 2 (g, 1.0 bar) H + (pH = ?)  Cl - (aq, 1.0 mol/L) Hg 2 Cl 2 (s) Hg(l), E = + 0.33 V 3. Using data from Appendix 2B in the text, calculate the standard potential for the half- reaction U 4+ (aq) + 4e - U(s) 4. Calculate Q for the cell reaction given the measured value of the cell emf. Balance the chemical equations by using the smallest whole-number coefficients: Pt(s) Sn 4+ (aq), Sn 2+ (aq)  Pb 4+ (aq), Pb 2+ (aq) C(gr), E = +1.33 V 5. Find the cell’s emf: Zn(s) Zn 2+ (aq, 0.37 mol/L)  Ni 2+ (aq, 0.059 mol/L) Ni(s) 6. A tin electrode in 0.015 M Sn(NO 3
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This note was uploaded on 09/28/2009 for the course GE 206E taught by Professor staff during the Spring '09 term at University of Texas.

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SUPPL INSTR FOR CH 302 (GE 206E) - AnswersPPgalvaniccells2...

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