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.

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Construct a galvanic cell from MnO4- (aq)/MnO2 (s) and H2 O2 (aq)/H2 O (l).a) Write a balanced equation for the cell.b) What is the value of E°cell?    standard Ni (s) | Ni2+ (aq) || Ag+ (aq) | Ag (s) is constructed and the standard cell potential is1.03 V.a) Write a balanced reaction for the cell.b) What is ∆G° for the cell?

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 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)

Name: NetID: 5. Determine the standard cell potential (in V to two decimal places) for the following redox reactions. 2+ (a) Al(s) | Al³+ (aq, 1 M) || Cu²+ (aq, 1 M) | Cu(s) (b) Al(s) + NO3(aq) + 4H+ (aq) - Al³+ (aq) + NO(g) + 2H₂O(1) 13+ A: 2.00 A: 2.62

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:

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)