Pt(s) |X' (aq), X2+, ELECTROCHEMISTRY: Pt(s) |X* (aq). (aq) || Y3+, *(aq) | Y(s) Given the line notation: where: 2+ + e° x+ E° = 0.48 V y3+ + 3 e → Y E° = -2.4 V Pt4+ + 4 e -→ Pt E° = 1.20 V Calculate the EMF.

Pt(s) |X' (aq), X2+, ELECTROCHEMISTRY: Pt(s) |X* (aq). (aq) || Y3+, *(aq) | Y(s) Given the line notation: where: 2+ + e° x+ E° = 0.48 V y3+ + 3 e → Y E° = -2.4 V Pt4+ + 4 e -→ Pt E° = 1.20 V Calculate the EMF.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A galvanic cell Mn(s)|Mn2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Mn electrode that weighs 34.9 g and a Pb electrode immersed in 532 mL of 1.00 M Pb2+(ag) solution. A steady current of 0.0519 A is drawn from the cell as the electrons move from the Mn electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Pb electrode gained when the cell is completely discharged? g (d) What is the concentration of the Pb2+(aq) when the cell is completely discharged? (Assume that the limiting reactant is 100% reacted.) M
Given the following reactions, AgBr(s) 2 Ag*(aq) + Br (aq) Ag (aq) + 2 CN (aq) 2 Ag(CN)2 (aq) Ksp = 5.8 x 10-13 Kf = 9.5 x 1021 determine the equilibrium constant for the reaction below. AgBr(s) + 2 CN (aq) ZAg(CN), (aq) + Br (aq)
For the cell shown, the measured cell potential, Ecell, is -0.3587 V at 25 °C. Pt(s) | H, (g, 0.839 atm) | H* (aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2 H* (aq) + 2 e H, (g) E° = 0.00 V Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V Calculate the Ht concentration. [H*] = %3D rIC ho C TV OLER EEDO DCD 24 4/2 DELL PrtScr Insert Home End F8 F9 F10 F11 F12 F4 F5 F6 F7
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What is the cell potential of the following electrochemical cell? (Report your answer to 2 significant figures.) Co(s) | Co²+ (aq, 0.31 M || Co²+ (aq, 0.035 M) | Co(s) Co²+/Co(s) = -0.28 V Eºred 1 2 4 7 +/- 5 8 v 3 6 9 0 X с x 100
Q1
9) At 25°C, what is the potential and the cell reaction for the following cell: Ni | Ni2+ (aq, 0010 M) || Cl(aq, 0.20M) | Cl2 (g, 1 atm) | Pt? What is the Keg at 298K?
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A galvanic cell is constructed in which the overall reac- tion is Cr,O} (aq) + 14 H¿O*(aq) + 6 I (aq) → 2 Cr* (aq) 1 3 I,(s) | 21 H,0(€) (a) Calculate AE° for this cell. (b) At pH 0, with [C»O3¯] = 1.5 M and [I-] = 0.40 M, the cell potential is found to equal 0.87 V. Calculate the concentration of Cr³*(aq) in the cell.
Pt(k)| Fe³+(aq), Fe²+(aq) // I-(aq) | 12(k) | Calculate the standard cell potential for the Pt(k) Cell and interpret whether the reaction taking place in the cell will proceed spontaneously under standard conditions. E° (Pt|Fe³+, Fe²+) = 0.77 V . E°( 12 | I-) = 0.53 V
The equilibrium constant for the reaction below is 4.0 x 10*12 at 298 K and 1 atm. CN (aq) + H30 (aq) = HCNaq) + H2O(1) When [HCN(aq)] = 1.0 M and (CN (aq)] = [H3O*(aq)] - 1.0 x 10 M, calculate AG In kl.