**Problem 2: Electrochemical Cell Calculation**Calculate \( E^\circ_{\text{cell}} \) for the following electrochemical cell:\[ \text{Ni(s)} | \text{Ni}^{2+} (\text{aq}) || \text{Hg}_2^{2+} (\text{aq}) | \text{Hg(l)} \]Given:- \( E^\circ_{\text{cathode}} = 0.79 \, \text{V} \)**Explanation:**This problem involves calculating the standard cell potential (\( E^\circ_{\text{cell}} \)) for a given electrochemical cell. The cell notation represents a galvanic cell with nickel metal and a mercury-based electrolyte. The reduction potential for the cathode (mercury half-cell) is given as 0.79 volts.

Given electrochemical cell : We have to calculate the E0cell for the above cell.

2- Calculate E° cell for the following electrochemical cell: Ni(s) | Ni2*(aq) || Hg2*(aq) | Hg(I) E° cathode = 0.79 V %3D

2- Calculate E° cell for the following electrochemical cell: Ni(s) | Ni2(aq) || Hg2(aq) | Hg(I) E° cathode = 0.79 V %3D

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...

See similar textbooks

Similar questions

4. The cell diagram for an electrochemical cell is given below: Mn(s) | Mn* (aq, 1.0 mol dm) || Ag* (aq, 1.0 mol dm)|Ag (s) In the above cell, the standard electrode potential of the silver hal f-cell is =0.80 V. E°cell = +1.98 V Write the equation for the reaction occurring at the anode and cathode. Write the overall cell equation Determine the standard electrode potential of the Mn2*/Mn half-cell What is the strongest oxidizing agent in the above cell? What is the strongest reducing agent in the above cell? a) 1) ii) b) i) i1) c) After the cell was used, the change in mass of the silver electrode was found to be 5.40 IS g Caleulate the change in mass of the manganese electrode.
What statement about a galvanic cell constructed with Cu*/Cu and Fe2*/Fe is correct? Standard reduction E°red, V potentials Cu* + e ---> Cu +0.52 Fe2+ + 2e ---> Fe |-0.44 O Fe2*(aq) is reduced at the cathode. O Fe(s) will reduce Cu*(aq). Fe(s) is a stronger oxidizing agent than Cu(s). O The standard cell potential (E°cell) is +1.40 V.
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.
Given: Half cell reaction E (V) Ag+(aq) + e- ---> Ag(s) 0.80 Cu+2(aq) + 2 e- ---> Cu(s) 0.34 Zn+2(aq) + 2 e- ---> Zn(s) -0.76 Ni+2(aq) + 2 e- ---> Ni(s) -0.23 (a) Pick up two of the above listed half-cells to build a voltaic cell that would have a maximum overall cell potential. Write the overall reaction equation. (b) Draw a detailed cell diagram and indicate which electrode is anode and which is cathode, and indicate the (-) electrode and the (+) electrode.
The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?+ (0.20 M) || H* (test solution)|H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn²+ is -0.76 V. (Enter your answer to two significant figures.) pH = %3!
6. The above diagram shows a Galvanic constructed from Ag|AGNO3(aq) and Ni|Ni(NO3)2(aq) half-cells and the half-cell electrode potentials are as follows: Ag*(aq) + e--> Ag(s); E° = 0.80 V %3! Ni2*(aq) + 2e --> Ni(s); E° = - 0.23 V Calculate the Ecell at 25°C when the electrolyte concentrations are: [Ag*] = 1.3 x %3D 10-4 M and [Ni2+] = 0.10 M. %3D
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
Standard Electrode Potentials at 25 °C Reduction Half-Reaction O Cu (aq) O H,Ozlaq) O Br O 10₂ (aq) Fyl) +20 H₂O₂(aq) + 2 H(aq) +2e" PbOg(s) +4 H(aq) +50, (aq) + 2 e Mn0 (aq) +4 H(aq) + 3 e MnO, (aq) +8H(aq) + 5 e Au³(aq) + 3 e PbOy(s) +4 H(aq) + 2e¯ C+20 00, (aq) +14 H(aq) + 6 e 00+ 4H*(aq) + 4 MnO₂ (s) +4 H(aq) +2e¯ 10₂(aq) + 6H(aq) +5e Big(0+20 VO₂ (aq) + 2 H(aq) + e¯ NO₂ (aq) + 4H(aq) + 3 e CO₂(0)+ Ag (ag)+e Fe(aq) + e 0)+2 H(aq) +2 e Mn0, (aq) + e (8) +26 Cu (aq) + e -2 (aq) -2 H₂O(0) Which of the following is the strongest oxidizing agent? -PbSO4(s) + 2 H₂O(0) →→MnO₂ (s) + 2 H₂O(0) Mn²(aq) + 4H₂O(1) - Au(s) ·Pb²+ (aq) + 2 H₂O(0) - 2 Cr (aq) 2 Cr³+ (aq) + 7 H₂O(1) → 2 H₂O( -2(aq) -Cu(s) Mn²+ (aq) + 2 H₂O(0) ₂(aq) + 3 H₂0(0) -2 Br (aq) - Vo²+ (aq) + H₂O( -NO(g) + 2 H₂O(1) — CIO; (aq) -Ag(s) -Fe²+ (aq) -) HyOz(ag) MnO₂ (aq) 1.00 0.96 0.95 0.80 0.77 0.70 0.56 0.54 0.52 E° (V) 2.87 1.78 1.69 1.68 1.51 1.50 1.46 1.36 1.33 1.23 1.21 1.20 1.09
For the galvanic cell at 298 K 2X(s) + 3Y2*(aq) –→ 2x3*(aq) + 3Y(s) E° cell = 0.39 V What is the measured cell potential (Ecell) when [Y2*] = 1.0 M and [X3+] = 0.01 M? Periodic Table and Datasheet O 0.39 V O 0.35 V O 0.43 V O 0.51 V
For the galvanic cell: Zn(s) + 2TI*(aq) 2TI(s) + Zn2*(aq) What is E°cel? Standard Electrode Potentials: Zn2*(aq) + 2e Zn(s) E° = -0.76 V TI*(aq) + eTI(s) E° = -0.34 V O 0.42 V O -0.42 V O 1.1 V O -1.1 V
5. What is voltage of the following cell? Sn(s) | Sn(NO3)2 (0.100 M) || AgNO3(0.020 M) | Ag(s)
Calculate the theoretical cell potential for the following galvanic cell: Mg | Mg2+ ( 1 M) || Cu2+ (2 M) | Cu