What is the standard cell potential for a galvanic cell that has the following half-reactions? Round the answer to 2 decimal places.MnO2(s) + 4H (ag) + 2eMn2+(aq) + 2H20()= 1.23 VPbCl2(s) + 2ePb(s) + 2CI (ag)= -0.27 VE° cllthe tolerance is +/-2%What is the net reaction for the cell? Include states in your answer.Edit

The standard cell potential or E° is the difference between the half cell potential at the cathode…

What is the standard cell potential for a galvanic cell that has the following half-reactions? Round the answer to 2 decimal places. MnO2(s) + 4H*(aq) + 2e o Mn2+(aq) + 2H20(/) = 1.23 V PbCl-(s) + 2e Pb(s) + 2CI"(aq) = -0.27 V E°cell = the tolerance is +/-2% What is the net reaction for the cell? Include states in your answer.

What is the standard cell potential for a galvanic cell that has the following half-reactions? Round the answer to 2 decimal places. MnO2(s) + 4H*(aq) + 2e o Mn2+(aq) + 2H20(/) = 1.23 V PbCl-(s) + 2e Pb(s) + 2CI"(aq) = -0.27 V E°cell = the tolerance is +/-2% What is the net reaction for the cell? Include states in your answer.

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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Using the Table of Standard Electrode Potentials (Appendix L, page 1251), calculate the E°cell for each of the following reactions and predict whether each redox reaction is spontaneous or non-spontaneous. 2. 3+, (a) Au(s) + NO; (aq) + 4H*(aq) → Au³*(aq) + NO(g) + 2H2O(); (b) Сu's) + 2Fe?" (ag) —> Сu?"(aq) + Fe(s) ; (c) 2Fe" (ag) + 21 (aд) —> I2(ад) + 2Fe?"(aq); 2+ (d) Zn(OH)2(s) + 4NH3(aq) → Zn(NH3)4*(aq) + 20H (aq);
Using the following half-cell equations and their standard electrode potentials: Fe"(aq) + e 5 Fc2"(aq) E' = +0.77 V Cu?"aq) + 2e 5 Cu(s) E = +0.34 V what is the cell diagram? A Pt|Fe?"aq), Fe"(aq) || Cu²"(aq) | Cu(s) B Cu (aq)| Cu(s) || Fe²"aq), Fe"(aq) | 32. Pt c Cu(s)|Cu²*(aq) || Fe²"aq), Fe*"(aq) | Pt D Pt| Fe"(aq), Fe²“aq) || Cu(s) | Cu²"(aq)
Calculate the cell potential for a Galvanic cell based on the reaction described by the following unbalanced equation at 25 C (assume standard, acidic conditions). Cu(s) + MnO4-(aq) -> Cu2+(aq) + MnO2(s)
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q19
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
Consider the following half-reactions: Half-reaction ° (V) Br2(1) + 2e → 2Br°(aq) |1.080V Sn²+ (aq) + 2e . Sn(s) |-0.140V Zn2*(aq) + 2e → Zn(s)|-0.763V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Br2(0) oxidize Zn(s) to Zn2*(aq)? (6) Which species can be oxidized by Sn2*(aq)? If none, leave box blank.
Consider the following half-reactions and their standard reduction potentials then give the standard line (cell) notation for a voltaic cell built on these half reactions. Mn2*(aq) + 2 e Mn(s) E° = -1.18 V Fe(aq) +3 e Fe(s) E° = -0.036 V A. Fe(s) | Fe3t(aq, 1.0 M) || Mn (s) | Mn 2*(aq. 1.0 M) B. Mn (s) | Mn 2*(aq, 1.0 M) | | Fe(s) | Fe(aq. 1.0 M) C. Fe(s) | Fe3t(aq. 1.0 M) || Mn2*(aq, 1.0 M) | Mn(s) D. Mn (s) | Mn 2*(aq. 1.0 M) || Fe(aq, 1.0 M) | Fe(s)
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.
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:
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn (aq)+Ba (s) Sn (s)+ Ba" (aq) 2+ Suppose the cell is prepared with 4.24 M Sn 2+ in the other. in one half-cell and 2.000 M Ba' Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
3) Draw a picture of the galvanic cell represented by the line notation below and then write the reduction half-reactions for each electrode. Also identify the anode and cathode for each half cell. Pt (s) | Fe3+ (aq), Fe2+ (aq) || Cr2O72-(aq), Cr3+ (aq), HA (aq) | Pt (s)