Consider a voltaic cell that operates from the following redox reaction: Cr2+ (aq) + Ag+ (aq) → Cr3+ (aq) + Ag (s) What is the value of Eocell if Eored(Ag1+/Ag) = 0.80 V and Eored(Cr3+/ Cr2+) = -0.41 V?
Question options:
A) Eocell = 0.39 V
C) Eocell = -1.21 V
D) Eocell = -0.39 V
E) Eocell = 1.21 V
Consider a voltaic cell that operates from the following redox reaction: Cr2+ (aq) + Ag+ (aq)...
Design a voltaic cell with the following two reduction half-reactions: Ag+(aq) + e− ⟶ Ag(s) Eo = 0.80 V Pb2+(aq) + 2 e− ⟶ Pb(s) Eo = −0.13 V Calculate Eocell and the equilibrium constant K for the voltaic cell at 298 K. Click here for a copy of Final Exam cover sheet.
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 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 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...
A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+ (aq) + Cr(s) + 3 Ce3+(aq) + Cr3+(aq) (a) What is the emf of this cell under standard conditions? X V (b) What is the emf of this cell when [Ce4+] = 1.9 M, [Ce3+] = 0.012 M, and [Cr3+] = 0.010 M? ху (c) What is the emf of the cell when [Ce4+] = 0.56 M, [Ce3+] = 0.80 M, and [Cr3+] = 1.3 M?...
QUESTION 13 Consider a voltaic cell based on the half-cells: Ag (aq) + e - Ag(s) E = +0.80 V Sn2+ (aq) + 2 e Sn(s) E = -0.14 V Identify the anode and give the cell voltage under standard conditions: O A Sn: Eºcell = -0.66 V B. Sn; Eºcell = 0.66 V O C. Ag: Eºcell = 0.67 V D. Ag: Eºcell = 0.94 V E. Sn; Eºcell = 0.94 V
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
1. A voltaic cell is constructed based on the following redox reaction: Sn2+ (aq) + Mn (s)àSn (s) + Mn2+ (aq) Calculate Ecell at 25 oC under the following conditions: (a) Standard conditions (b) [Sn2+] = 0.0200 M; [Mn2+] = 4.00 M (c) [Sn2+] = 0.500 M; [Mn2+] = 0.00250 M 2. Consider the following redox reaction at 25oC: MnO2 (s)àMn2+ (aq) + MnO4- (aq) (a) Balance the equation in acid (b) Calculate Eocell (c) CalculateDGorxn (d) Calculate K Hint!!!...
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 =...
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...