Here Ag is more powerfull oxidizing agent than Fe and hence Ag will act as cathode. So correct option is (A).
What is the cathode reaction for the spontaneous process associated with this voltaic cell? Ag^+(aq) +...
What is the standard cell potential (Y) for the spontaneous voltaic cell formed from the given half-reactions? Reduction Half-Reaction Ered (V) Anode -0.41 Fe2+ (aq) + 2e Fe(s) Cl2 (8) +20 +2 (aq) Cathode 1.36
Reaction Eo Ag+(aq)+ e-→ Ag(s) 0.80V Zn2+(aq)+ 2e-→Zn(s) -0.76V What would be the cathode reactant in the Voltaic Cell made from the half-reactions above? Question options: a. Zn2+(aq) b. Ag+(aq) c. Ag(s) d. Zn(s)
38. The following redox half reactions are combined in a voltaic cell. Which reaction occurs at the cathode and what is the Eceu? Fe2+(aq) + 2e → Fe(s) E°=-0.44 V Cu²+(aq) + 2e → Cu(s) E°= 0.34 V a) b) c) d) Cu2+(aq) + 2e → Cu(s), Ecell = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecel = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecell =-0.10 V Cu²+(aq) + 2e → Cu(s), Ecel = 0.10 V Cu²+ (aq) +...
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,...
For the spontaneous chemical reaction that takes place in a voltaic cell, the sign of AG is and electrons flow from the to the a) negative, anode, cathode b) positive, anode, cathode c) negative, cathode, anode d) positive, cathode, anode a
Enter electrons as e A voltaic cell is constructed from a standard Fe? Fe half cell (Ered -0.440V) and a standard Izt half cell (Ered -0.535V). (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is Enter electrons as e. Use smallest possible integer coefficients. If a...
A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag + (aq) → Cu 2+ (aq) + 2 Ag(s) The Eº cell 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...
A voltaic cell is based on the reduction of Ag^+(aq) to Ag(s) and the oxidation of Sn(s) to Sn^2+(aq). (a) Write half-reactions for the cell's anode and cathode. Include the phases of all species in the chemical equation. Anode Cathode (b) Write a balanced cell reaction. Include the phases of all species in the chemical equation.
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
A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag + (aq) → Cu 2+ (aq) + 2 Ag(s) The Eº cell 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...