Consider the following electrochemical cell at 298 K where the source ofCu2+ (aq) is the sparingly soluble salt CuX.Zn(s)|Zn²* (aq, 0.50M)||Cu²+ (aq)|Cu(s)Zn2* + 2e = Zn E° = -0.76 VCu2+ + 2e = CuE° = 0.34 VIf the potential created from this cell = 1.03 V, what is Ksp for CuX?O 1.9x10-93.8x10 124.6x10 62.0x10 7

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Answered: Consider the following electrochemical…

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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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
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
If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 2 significant digits.
For the galvanic (voltaic) cell Fe(s) + Mn²⁺(aq) ⟶ Fe²⁺(aq) + Mn(s) (E° = 0.77 V at 25 °C), what is [Fe²⁺] if [Mn²⁺] = 0.030 M and E = 0.78 V? Assume T is 298 K
Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing indium and cadmium. In(s)||In3+(aq)‖‖Cd2+(aq)||Cd(s)In(s)⁢|In3+⁢(aq)‖Cd2+⁢(aq)|Cd(s) anode: cathode: net cell reaction:
For the cell: Zn(s) + 2H† (aq) →→ Zn2+(aq) + H2 (g) If [Zn2+] = 1 M, PH2 = 1 atm, and E = 0.123 V what is pH?
Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions are provided for each metal: Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V Given that the standard cell potential is 0.019 V and the overall equation is 2 Cr³⁺ (aq) + 3 Zn (s) → 2 Cr (s) + 3 Zn²⁺ (aq), what is the cell potential for this cell at 25 °C when [Zn²⁺] = 0.0323 M and [Cr³⁺] = 0.1736 M?
A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni²+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28
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
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e - Zn(s) :-0.763 V (red |Cro (aq)+4 H2O(1)+3e Cr(OH)3(s)+5OH (aq) :-0.13 V = - (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.
Which of the following reactions occurs at the anode of an electrochemical cell composed of Zn│Zn2+(aq) and Fe│Fe2+(aq) half-cells? Their reduction potentials are as follows: Zn2+ + 2e– --> Zn; Eo = -0.763 V Fe2+ + 2e– --> Fe; Eo = -0.447 V (A) Zn2+ + 2e– --> Cr; (B) Zn --> Zn2+ + 2e–; (C) Fe --> Fe2+ + 2e–; (D) Fe2+ + 2e– --> Fe;

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