What is the cell notation of a cell with no liquid junction and with thefollowing half-reactions?2Hg(1) + 2CI¯ → Hg2Cl2(s) + 2eCl2(g) + 2e¯ → 2CI¯CO Pt| Hg(1) | Hg2Cl2(s) | HCI | Cl2{g) | PtO Pt| Hg(1) | Hg2Cl2(s) || HCI | Cl2(g) | PtO Pt| Cl2(g) | HCI || Hg2Cl2(s) | Hg(l) | PtO Pt| Cl2(g) | HCI | Hg2Cl2(s) | Hg(1) | PtO Pt | Cl2(g) | HCI | Hg2Cl2(s) || Hg(1) | Pt

Given cell reactions are : 1). 2Hg (l) + 2Cl- (aq) -------> Hg2Cl2 (s) + 2e- 2). Cl2 (g) + 2e-…

Answered: What is the cell notation of a cell…

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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Prepare a sketch and write the half-reactions and overall cell reaction for the electrochemical cell designated by: Pt(s) | Ag(s) |AgCl(s) | Cl-(a = 1) | Cl2(g, 1 bar)| C(graphite) | Pt(s)
What is the balanced overall reaction of the following cell? Ag(s)|Ag+(aq)||Mg2+(aq)|Mg(s) Group of answer choices: 2 Ag(s) + Mg2+(aq) → 2 Ag+(aq) + Mg(s) Ag(s) + Mg 2+(aq) → Ag+(aq) + Mg(s) 2 Ag+(aq) + Mg(s) → 2 Ag(s) + Mg2+(aq) Ag+(aq) + Mg(s) → Ag(s) + Mg2+(aq)
Calculate the cell potential of each of the following electrochemical cell at 25oC. a. Pt|H 2 (8.00 atm)|H + (1.00 x 10 -3 M)‖Ag + (0.00549 M)|Agb. Pt|H 2 (1.00 atm)| H + (pH = 5.97 ) ‖ H + (pH=3.47)|H 2 (1.00 atm)|Ptc. Pt|H 2 (0.0361 atm)|H + (0.0175 M)‖H + (0.0175 M)|H 2 (5.98 x 10 -4 atm)|Pt Please solve and give explanations steps.
Calculate AG for the following cell reaction: Tl(s) | Tl+ (aq) || Ni²+ (aq) | Ni(s) From AG, determine the standard potential for the half-reaction Tl+ (aq) + e → Tl(s) AG; for Tl+ (aq) is -32.4 kJ/mol. 2+ AG; for Ni²+ (aq) is -45.60 kJ/mol. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction Ni²+ (aq) + 2e Ni(s) AG = J Standard Potential, E° (V) -0.23 Standard reduction potential for the half-reaction = V
Silver metal can be dissolved in acidic solutions via a redox reaction with generation of hydrogen gas. Which of the following is the correct cell notation for the reaction that will occur?
Write a balanced equation for the overall cell reaction in the following galvanic cell and tell why inert electrodes are required at the anode and cathode. Pt(s) | Br (aq) | Br₂ (1) || Cl; (g) | Cl(aq) | Pt(s)
Give the standard line notation for each cell. (a) 2 IO3 (aq) + 10 Fe2+ (ag) + 10 H* (aq) = 10 Fet (ag) + I2 (aq) + 5 H2O(1) O Pt(s) | Fe?+ (aq), Fe+ (ag) || IO3 (ag), Ht (ag), I2 (ag) | Pt(s) O Pt(s) | Fet (aq), I2 (ag) || Fe2+ (ag), IO3 (ag), H* (ag) | Pt(s) Pt(s) | IO3 (ag), H* (ag), I2 (aq) || Fe2+ (ag), Fet (ag) | Pt(s) Pt(s) | Fe2+ (ag), IO3 (ag), H* (aq) || Fet (aq), I2 (ag) | Pt(s) (b) Zn(s) + 2 Ag* (ag) = Zn?+ (aq) + 2 Ag(s) O Zn(s) | Zn?+ (aq) || Ag* (aq) | Ag(s) O Zn(s) | Ag* (aq) || Zn?+ (ag) | Ag(s) Ag(s) | Ag* (ag) || Zn2+ (aq) | Zn(s) O Ag(s) | Zn?+ (aq) || Ag* (aq) | Zn(s) (c) H2O2 (aq) + 2 H* (ag) + 2 e → 2 H2O(1) E = 1.78 V 02 (9) + 2 H* (ag) + 2 e + H2O2 (ag) E = 0.68 V O Pt(s) | O2(9) | H2O2 (aq), H* (ag) || H2O2 (ag), H* (ag) | Pt(s) Pt(s) | H2O2 (aq), H* (ag) || O2 (9) | H2O2 (ag), H* (ag) | Pt(s) Pt(s) | H2O2 (aq) | O2(9) || H* (aq) | Pt(s) O Pt(s) | H2O2(aq) | Pt(s) (d) Mn2+ (aq) + 2 e → Mn(s) E° = - 1.18 V Fe+ (aq) + 3 e → Fe(s) E - -0.036 V O Mn(s) | Mn²+ (ag)…
Calculate Eu for the following cell: Pt(s) | H₂(g) | H *(aq) || Pb2+ (aq) | PbSO4(s) | Pb(s) given the following standard reduction potentials. 2 H(aq) + 2e →→ H₂(g) PbSO4(s) + 2e →→ Pb(s) + SO42 (aq) O a. -0.712 V O b. +0.356 V O c. -0.356 V O d. +0.712 V O e. -0.178 V E° = 0.000 V E = -0.356 V
Consider this cell diagram for an electrochemical cell: Pt(s) | H2(g) | H*(aq) || Cu*(aq) | Cu(s) What is the overall balanced reaction for this redox reaction? O 2H (aq) + 2Cu(s) H2(g) + 2Cu (aq). O H2(g) + 2Cu'(aq) → 2H*(aq) + 2Cu(s) O H2(g) + 2Cu(s)H'(aq) + 2Cu'(aq) O H2(g) + Cu (aq) H'(aq) + Cu(s)
Balance the REDOX reaction associated with the cell shown below, in acidic medium: 2+ Fe(s) | Fe² || MnO (aq) Mn²) | Pt(s) Μη '(aq) 4(aq)' Enter the number for the coefficient of H₂O in the balanced equation:
Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg²+ (aq) and a cathode where Cr³+ (aq) is reduced to Cr²+ (aq) at a platinum electrode. Assume all aqueous solutions have a concentration of 1 mol/L. Mg(s)| Mg2+ (aq)|| Cr³+ (aq)| Cr²+ (aq)| Pt(s)
What is the balanced equation for the galvanic cell reaction expressed using the following shorthand notation? Mg (s) | Mg2+ (aq) || Cl2 (g) | Cl– (aq) | C (s)

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