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Question 6 (1 point) Transpose the following redox reaction into cell notation. Mg (s) + Pb2+...
Question 5 (1 point) Transpose the following galvanic cell into cell notation. Anode: Iron metal in a 1.0 M solution of Fe(NO3)2 Cathode: Cobalt metal in a 1.0 M solution of Co(NO3)2 O1 Pt (s)| Fe3+ (1 M), Fe2+ (1 M) || Co(NO3)2 (1 M) Co (s) I O Co (s) | Co(NO3)2 (1 M) || Fe(NO3)2 (1 M) Fe (s) O Fe (s) Fe(NO3)2 (1 M) || Co(NO3)2 (1 M) | Co (s) O Co (s) | Co(NO3)2 (1...
Question 4 (1 point) What is the Eºcell for the spontaneous electrochemical cell between Pb2+/Pb and Mg2+/Mg? O +2.23 V -2.36 V O - 2.23 V +2.36 V Show Report 07 CRAIN605 PAS lenovo
What is undergoing reduction in the redox reaction represented
by the following cell notation?
Pb(s) | Pb2+(aq) | | H+(aq) H2 | (g) | Pt
A. Pb(s)
B. Pt
C. Pb2+(aq)
D. H2(g)
E. H+(aq)
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Question 7 (1 point) Consider the following cell: Pb(s) | PbSO4(s) S042-(aq) || Pb2+(aq) | Pb(s) The reaction utilized by this cell is O Pb(s) + 2H+(aq) --> Pb2+(aq) + H2(g) O s042-(aq) + H+(aq) --> HSO4-(aq) O PbSO4(s) --> Pb2+(aq) + SO42-(aq) O Pb2+(aq) + SO42- (aq) --> PbSO4(s) O s042-(aq) + H20(1) --> HS04"(aq) + OH(aq)
Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg2+ (aq) and a cathode where Pb2+ (aq) is reduced to Pb (s) . Assume all aqueous solutions have a concentration of 1 mol/L.
tion 3 of 40 ) A voltaic cell employs the redox reaction: Zn (s) + Pb2+ (aq) — Zn2+ (aq) + Pb () where Pb2+ (aq) + 2e Zn2+(aq) + 2e Pb(s) E = -0.1262 V Zn(s) E = -0.7618 V The cell potential (Ecell) of this voltaic cell when [Pb2+1 = 1.10 M and [Zn2+) = 0.00110 Mis:
A voltaic cell employs the following redox reaction: 2 Fe3+ (aq) + 3 Mg(s) + 2 Fe (s) + 3 Mg²+ (aq) Calculate the cell potential at 25 °C under each of the following conditions. Part B [Fe3+] =1.3x103 Μ; [Mg2+] = 1.85 M ΡΟΙ ΑΣΦ 5 - 0 ΕΞΙ ? Ecell = - Part [Fe3+] = 1.85 M ; (Mg2+] = 1.3x10-3 M 1190 AM O O ? Ecell =
When the Pb2+ concentration is 1.17 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.356V. What is the Mg2+ concentration? Pb2+(aq) + Mg(s) Pb(s) + Mg2+(aq) Answer: _____M
Consider the following unbalanced equation. Pb(s) + Mg2+(aq) right --> Mg(s) + Pb2+(aq) (a) What are the following standard voltages? Include the sign, changing it as appropriate. Use the standard reduction potentials in the Reference Tables. Enter the number of decimal places allowed by the data in the table. -standard oxidation potential for the oxidation half-cell: ___ V -standard reduction potential for the reduction half-cell: ___ V -potential for the entire cell:___ V (b) Select all that apply for the...
4. A voltaic cell employs the following redox reaction: 2 Fe3+(aq) + 3 Mg(s) → 2 Fe(s) + 3 Mg2+(aq) What is the number of electrons that have been transferred in this redox reaction? 5. Use the following reduction potentials to determine if the reaction in Question 4 represents a voltaic or electrolytic cell and if the reaction is spontaneous or non-spontaneous. Fe3+(aq) + 3 e−(aq) → Fe(s) Eo = −0.036 V Mg2+(aq) + 2 e−(aq) → Mg(s) Eo =...