1Determine Eº for a galvanic (voltaic) cell ifAG° = -3.2 kJ/mol and n = 3. (F = 96,500J/(V.mol))47+/-2LO5Question 11 of 158| V369OSubmitTap here or pull up for additional resourcesXCx 10 □

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L 1 Determine Eº for a galvanic (voltaic) cell if AG° = -3.2 kJ/mol and n = 3. (F = 96,500 J/(V.mol)) 4 7 +/- 2 5 Question 11 of 15 8 | V 3 6 9 0 Submit Tap here or pull up for additional resources X C x 100

L 1 Determine Eº for a galvanic (voltaic) cell if AG° = -3.2 kJ/mol and n = 3. (F = 96,500 J/(V.mol)) 4 7 +/- 2 5 Question 11 of 15 8 | V 3 6 9 0 Submit Tap here or pull up for additional resources X C x 100

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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eq eq creq 2req #m 3 Use the References to access important values if needed for this question. A standard galvanic cell is constructed in which a Co2+ | Co half cell acts as the cathode. Which of the following statements are correct? 0 E Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) In the external circuit, electrons flow from the other compartment to the Co²+ | Co compartment. 0 1211 could be the other standard half cell. D The cathode reaction is Co-> Co2+ + 2e². As the cell runs, anions will migrate from the other compartment to the Co2+ | Co compartment. 0 The anode reaction could be Al-> Al³+ + 3e. Submit Answer $ 4 R F 07 20 Retry Entire Group 9 more group attempts remaining % 5 Cengage Learning Cengage Technical Support T G 6 MacBook Pro Y B & 7 H U N * 00 8 J I ( 9 K M € ) O 0 8 L + Save and Ex = [
A voltaic cell consists of Co I Co?²*(0.25 M) II Cu²*(0.35M) I Cu. The electrode potential at this concentration is [A] 0.6157V [B] 0.6025 V [c]0.6243V [D] 0.5014 V (Co* + 2 e→ Co, ɛ°red = -0.28 V, Cu²* +2 e→ Cu, ɛ°red = +0.34 V) A C O D
For the galvanic cell at 298 K Zn(s) + 2ln2+(aq) --> Zn²*(aq) + 2ln*(aq) cell = 0.36 V What is the equilibrium constant, K? Item equation/constant: F = 96470 J/V• mol e- R = 8.314 J/(mol·K) %3D RT E° =" InK nF Select one: O a. 1.2x106 O b. 8.3x10-7 c. 6.8x10-13 O d. 1.5x1012
5. * A voltaic cell consists of Co I Co"(0.25 M) II Cu" (0.35M) I Cu. The electrode potential at this concentration is [A] 0.6157 V [B] 0.6025 V [C]0.6243 V [D] 0.5014 V (Co* + 2 e> Co, s°red = -0.28 V, Cư* +2 e> Cu, s°red = +0.34 V) [A] [B] O [C) [D]
both questions go together... thanks! Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e- 2 Br-(aq) 1.08 NO3-(aq) + 4 H+(aq) + 3 e- NO(g) + 2 H2O(l) 0.96 2 Hg2+(aq) + 2 e- Hg22+(aq) 0.920 Hg2+(aq) + 2 e- Hg(l) 0.855 Ag+(aq) + e- Ag(s) 0.799 Hg22+(aq) + 2 e- 2 Hg(l) 0.789 Fe3+(aq) + e- Fe2+(aq) 0.771 I2(s) + 2 e- 2 I-(aq) 0.535 Fe(CN)63-(aq) + e- Fe(CN)64-(aq) 0.48 Cu2+(aq) + 2 e- Cu(s) 0.337 Cu2+(aq) + e- Cu+(aq) 0.153 S(s) + 2 H+(aq) + 2 e- H2S(aq) 0.14 2 H+(aq) + 2 e- H2(g) 0.0000 Pb2+(aq) + 2 e- Pb(s) -0.126 Sn2+(aq) + 2 e- Sn(s) -0.14 Ni2+(aq) + 2 e- Ni(s) -0.25…
MISSED THIS? Read Section 20.6 (Pages 917-922) A voltaic cell consists of a Zn|Zn²+ (E° = -0.76 V) half-cell and a Ni Ni²+ (E° = -0.23 V) half-cell at 25 °C. The initial concentrations of Ni²+ and Zn²+ are 1.70 M and 0.100 M. respectively. The volumes of the half-cells are the same. Part A What is the initial cell potential? Express your answer in volts to two decimal places. Ecell = Submit Part B Ecell = ΠΑΠ ΑΣΦ Submit Request Answer What is the cell potential when the concentration of Ni²+ has fallen to 0.600 M? Express your answer in volts to two decimal places. ΓΙ ΑΣΦ ? Request Answer V ? V
2req A voltaic cell is constructed from a standard Sn*Sn half cell (Eo 2+ -0.140V) and a standard Cr* Cr half cell (E red red =-0.740V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) 2req The anode reaction is: s 2req OMD The cathode reaction is: OM) s 2req OMD The spontaneous cell reaction is: ts 2req OM) ts The cell voltage is V.
5a
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Enter electrons as e". A voltaic cell is constructed from a standard Pb²+|Pb half cell (E° red = -0.126V) and a standard Crt Cr+ half cell (E° = -0.410V). red (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: + The spontaneous cell reaction is: + The cell voltage is V. + 1 1
c) 45.8 kJ/mol 9. Using the appropriate half-cell reactions, and assuming y. - product of AgCl at 25°C: AgCl(s) Ag'(aq) + Cl(aq) a) 5.21 x 10-13 b) 1.68 x 10-10 1.85 × 10-10 10. Between 0°C and 90°C th d) 50.7 kJ/mol 1, calculate the solubility d) 1.56 × 10-10