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Design a voltaic cell with the following two reduction half
-reactions :
Design a voltaic cell with the following two reduction half-reactions Ag+(aq) + e-→ Ag(s) Zn2+(aq) + 2 e-→Zn(s) E 0.80 V Eo = 0.76 V Calculate Eocell and the equilibrium constant K for th copy of Final Exam cover sheet. e voltaic cell at 298 K. Click here for a E° cell -0.04 V and K-4.7 E cell-0.04 V and K-0.21 O Eocel =-0.04 V and K =...
What is the net cell reaction for the cobalt-silver voltaic cell? Co(s)→Co3+(aq)+3e− Ag+(aq)+e−→Ag(s)
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) – Cu 2+ (aq) + 2 Ag(s) The E° for the reaction is +0.46 V. The initial (nonstandard) conditions are: [Ag +] = 0.025M; [Cu 2+] = 2.0 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is the cell potential,...
A voltaic cell is made from Ni(s), Ni2+(aq), Ag(s) and Ag+
a. Fill in the diagram with the chemicals associated with each
part of the cell.
b. Write a balanced cell reaction
A voltaic cell is made from Ni(s), Niz*(aq), Ag(s) and Ag 7. a. Fill in the diagram with the chemicals associated with each part of the cell. Ni2+ + 2 e-→ Ni(s) Ag+ + e-→ Ag(s) -0.25 0.80
Consider the reaction corresponding to a voltaic cell and its standard cell potential. cell Zn(s) + Cu2+ (aq) + Cu(s) + Zn2+ (aq) E = 1.1032 V As What is the cell potential for a cell with a 2.573 M solution of Zn²+ (aq) and 0.1055 M solution of Cu²+ (aq) at 432.4 K?
all parts please
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) Cu 2+ (aq) + 2 Ag(s) The E° for the reaction is +0.46 V. The initial (nonstandard) conditions are: (Ag +) = 2.0 M; [Cu 2+] = 0.025 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is...
A voltaic cell is constructed from an Ni2+ (aq) -Ni(s) half-cell and an Ag+ (aq)- Ag(s) half-cell. The initial concentration of Ni2+ (aq) in the Ni2+ - Ni half-cell is [Ni2+1 = 1.80x10-2 M. The initial cell voltage is +1.13 V. Part A By using data in Table 20.1 in the textbook, calculate the standard emf of this voltaic cell. V AEQ ? E V Submit Request Answer Part B. Will the concentration of Ni2+ (aq) increase or decrease as...
6. Consider a voltaic cell based on the following cell reaction: Ni(s) + At2(s) ? Ni2+(aq) + 2At– (aq) Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine? [E°(Ni2+/Ni) = –0.25 V]
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu?+ (aq) Cu(s) + Zn²+ (aq) E cell 1.1032 V What is the cell potential for a cell with a 2.344 M solution of Zn?' (aq) and 0.1701 M solution of Cu?+ (aq) at 441.2 K?
Consider a voltaic cell based on the half-cells: Ag+ (aq) + e - Ag(s) E* = +0.80 V Pb2+(aq) + 2 e-Pb(s) E* = -0.13 V Identify the anode and give the cell voltage under standard conditions: = 0.67 V Ag: E cell B. Pb: E cell = 0.67 V OC. Pb: E cell = 0.93 V D. Pb: E cell = -0.67 V E. Ag: E cell = 0.93 V