A voltaic cell consists of two half-cells La/La3+ and Sn/Sn2+. The concentration ofSn2+ is 8.00 M. The observed voltage for the cell is 2.293 V at 25°C.What is the molar concentration of La3+ in the cell?Sn2+(aq) +2e-Sn(s)E°--0.14VLa 3+(aq) +3e- a(s) E°--2.38V(Do not enter units, use 3 significant figures in the answer. Do not use scientific notation)Your Answer:

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Answered: A voltaic cell consists of two…

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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Find the FALSE statement about the voltaic cell based on the two reduction half- reactions shown below. The concentrations of the ions are [Al3+] = 0.01 M, [Mn2*] = 0.1 M. A13+(aq) + 3e¯ - Al(s) E°red = -1.66 V Mn2+(aq) + 2e - Mn(s) E°red = -1.18 V Al(s) is a stronger reducing agent than Mn(s) The observed cell potential is 0.49V For the balanced equation, n = 6 and Q = [AI³+]/ [Mn2+]. Using base 10, logQ = -1. The shorthand diagram for this cell is Al(s) | AI3*(aq) || Mn²*(aq) | Mn(s).
the standard cell potential (E°cell) for the voltaic cell based on the reaction below is what? Cr(s) + 3Fe3+(aq) --> 3Fe2+(aq) + Cr3+(aq)
which reaction could be used to generate electricity in a voltaic electochemical cell at the standard conditton ? a) Pb2+(aq) + Mg(s) --> Pb(s) +Mg2+(aq) b) Zn2+(aq) + Sn(s) --> Zn(s) + Sn2+ (aq) c) NaCl(aq) + AgNO3(s) --> AgCl(s) + NaNO3(aq) d) Cu2+(aq) +4NH3(aq) --> Cu(NH3)4^2+(aq) e) none of the above please explain
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
Four voltaic cells are set up. In each, one half-cell contains a standard hydrogen electrode (SHE). The second half-cell is one of the following. 2+ • Cr" (aq, 1.0 M) | Cr(s) 3+ Al" (ag, 1.0 M) | Al(s) 2+ • Ca" (aq, 1.0 M) | Ca(s) 2+ Hg2" (aq, 1.0 M) | Hg(1) (a) In which of the voltaic cells does the hydrogen electrode serve as the cathode? 2+ O SHE & Cr´" (aq, 1.0 M) | Cr(s) ,3+ O SHE & Alº" (aq, 1.0 M) | Al(s) 2+ O SHE & Ca" ' (aq, 1.0 M) | Ca(s) 2+ O SHE & Hg," (aq, 1.0 M) | Hg(1) (b) Which voltaic cell produces the highest voltage? Which produces the lowest voltage? The highest voltage will be produced by combining the SHE and the half-cell. The lowest voltage will be produced by combining the SHE and the v half-cell.
8
What would be produced by an electrolytic cell involving the following half-reactions: Pb2+(aq) + 2e- → Pb(s) E° = -0.13 V2H+(aq) + 2e- → H2(g) E° = 0.00 V a)Pb2+(aq) and H+(aq) b)Pb2+(aq) only c)Pb2+(aq) and H2(g) d)Pb(s) only e)Pb(s) and H+(aq) f)H+(aq) only g)Pb(s) and H2(g)
consider a voltaic cell with the overall reaction zn + 2ag+ zn2+ + 2ag what will the value of e cell (v) be when [ag+] =1.9 m and zn 2+ = .003m Ag^+ + e- -> Ag(s). E red = 0.80V zn2^+ + 2e^- -> Zn (s) E red = -0.76 V
3) Use half cell potentials to determine if each reaction occur spontaneous in the direction written (yes/no). a) Ca¹2(aq) + Zn(s) - Ca(s) + Zn¹²(aq) b) Au*³(aq) + Ag(s) - Au(s) + Ag (aq) c) Co(s) + Pb (aq) - Co²(aq) + Pb(s) d) Pb(aq) + H₂S(g) -Pb¹2(aq) + S(s) ing if each metal will dissolve in 1M HCl.
Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the concentrations. Sn(s) Sn+ (aq, 0.0155 M) Ag*(aq., 1.50 M) Ag(s) net cell equation: Sn(s) +2Ag*(aq) - Sn2+ (aq) + 2Ag(s) Calculate E and Ecell at 25 °C, using standard potentials as needed. V 0.96 %3D Ecell V Ecell 0.876 %3D Incorrect
Use the standard reduction potentials given below to predict if a reaction will occur between Sn(s) and F2(g) , when the two are brought in contact via standard half-cells in a voltaic cell. F2(g) + 2e- --> 2F-(aq) E°red = 2.870 V Sn2+(aq)+ 2e- ---> Sn(s) E°red = -0.140V If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.______+_______----->______+_______

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