Answered: 10. What is the standard cell potential…

10. What is the standard cell potential of the following electrochemical cell at 25°C: Ni(s) I NiCl2(aq) || Cu(NO3)2 (aq) | Cu(s) a. 0.62 V b. -0.62 V c. 0.60 V d. -0.60 V e. 0.095 V at r

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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11. Consider the following reaction and its AG-AG• at 25.00 °C. 12 Coeside 2Ag*(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG =-88660 J/mol a. Calculate the standard cell potential, Ecellº, for the reaction. b. Calculate the equilibrium constant, K, for the reaction. Wtoxided what is reduced? CLEAREY
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
Given the following two half-reactions, determine which overall reaction is spontaneous, and calculate its standard cell potential. Cd2*(aq) + 2 e- Cd(s); E° = -0.403 V Zn2"(aq) + 2 e-Zn(s); E° = -0.763 V O A. Cd(s) + Zn2*(aq) OB. Cd(s) + Zn(s)¯ OC. ca²*(aq) + Zn²*(aq)' Cd2+(aq) + Zn(s); E° = -0.360 V Cd2*(aq) + Zn²+(aq); E° = -1.166 V PCd(s) + Zn(s); E° = +1.166 V O D. Cd2+(aq) + Zn(s) cd(s) + Zn2*(aq); E° = +0.360 V
For the galvanic cell: Zn(s) + 2Tl+(aq) 2Tl(s) + Zn2+(aq) Eocell = 0.42 V The standard reduction potential for the half cell Zn2+(aq) + 2e– Zn(s) is Eored = –0.76 V What is the standard reduction potential for Tl+(aq) + e– Tl(s) Eored = ? V a. +0.17 V b. –0.17 V c. –0.34 V d. +0.34 V
e. Calculate the cell potential Ecell of the Galvanic cell (25°C). Give your answer in volts (V).
Consider the following electrochemical cell at 298 K where the source of Cu2+ (aq) is the sparingly soluble salt CuX. Zn(s)|Zn²* (aq, 0.50M)||Cu²+ (aq)|Cu(s) Zn2* + 2e = Zn E° = -0.76 V Cu2+ + 2e = Cu E° = 0.34 V If the potential created from this cell = 1.03 V, what is Ksp for CuX? O 1.9x10-9 3.8x10 12 4.6x10 6 2.0x10 7
The following reaction is non-spontaneous as written when the components are in their standard states, the cell potential is -0.16 V. Which of the following is true? Co(s) + Fe²*(aq) 2 Co²* (aq) + Fe(s) E =-0.16 V A. the reaction is spontaneous if [Co2+/[Fe2+] > 3.91x10-6 В. the reaction is spontaneous if [Co2+]/[Fe2+] -6 C. the reaction is spontaneous if [Co2+/[Fe2*] > 2.56x105 D. the reaction is spontaneous if [Co2*]/[Fe2+] 5
Calculate the K and AG for the following reaction at 25 °C: с Zn(s) + CuSO₂ (aq) = ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °℃ and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. K с Part 2 of 2 = AGO = x10 Round your answer to 4 significant digits. kJ mol X Ś x10
Given the following standard reduction half reactions calculate the standard cell potential (E°cell) to 2 decimal places. O2(g) + 4H+ + 4e" 1 4H* (aq) 2H20L) ; E°red. = 1.23 V A13+ (aq) + Зе Al(s) ; E°red. = -1.66 V
In the electrochemical cell shown here, the concentrations of Mn2+ and Cr3+ are 1.5x10-5 and 0.25 mol L-1, respectively. What is the cell potential? = E 0.0257 V -InQ KNO, Mn Mn(NO3)2 Cr(NO3)3 Mn* (aq) + 2e 2 Mn(s) E° =-1.18 V Cr* (aq) + 3e¯ 2 Cr(s) E° =-0.74 V
Calculate the theoretical cell potential for the following galvanic cell: Mg | Mg2+ ( 1 M) || Cu2+ (2 M) | Cu