If the following half-reactions are used in an electrolytic cell: Ag+(aq) + e− ⟶ Ag(s) Eo...
If the following half-reactions are used in an electrolytic cell: Ag+(aq) + e− ⟶ Ag(s) Eo = 0.80 V Ca2+(aq) + 2 e− ⟶ Ca(s) Eo = −2.76 V Click here for a copy of Final Exam cover sheet.
1) The metal solid that is plated out at the cathode is [Ag(s), Ca(s)]
2) It would take [3, 8. 16] hours to deposit 60 g of the solid with a current of 5.0 A.
Homework Answers
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If the following half-reactions are used in an electrolytic
cell: Ag+(aq) + e− ⟶ Ag(s) Eo...
Design a voltaic cell with the following two reduction half-reactions: Ag+(aq) + e− ⟶ Ag(s) Eo =...
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.
Design a voltaic cell with the following two reduction half -reactions : Design a voltaic cell...
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 =...
5. Consider the following set of half reactions Ag (aq)Ag (s) Cu2(a)2 e- Cu (s) Ai...
5. Consider the following set of half reactions Ag (aq)Ag (s) Cu2(a)2 e- Cu (s) Ai (aq)3eAl (s) Eo0.7996 V E0.342 V Eo-1.6632 V i. Which pair of half reactions would make the battery with the largest E cell? i. Identify the cathode and the anode for this battery, and calculate the value of E cell. i. Write the overall redox reaction that would take place in the battery above.
Consider the two reduction half-reactions: Br2(l) + 2 e− ⟶ 2 Br−(aq) Eo = 1.09 V...
Consider the two reduction half-reactions: Br2(l) + 2 e− ⟶ 2 Br−(aq) Eo = 1.09 V Ag+(aq) + e− ⟶ Ag(s) Eo = 0.337 V Use the electrode potentials above to calculate Eocell and ∆Gorxn for the reaction below, and determine if it is the reaction for a voltaic cell or an electrolytic cell.
An electrochemical cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that...
An electrochemical cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Cu(s) and Cu2+(aq). What species are produced at the electrodes under standard conditions? E° = +0.80 V Agt(aq) + e- → Ag(s) Cu2+(aq) + 2 e- → Cu(s) E° = +0.34 V O Ag(s) is formed at the cathode, and Cu(s) is formed at the anode. Ag(s) is formed at the cathode, and Cu2+ (aq) is formed at the anode. Cu(S) is formed...
Consider the 2 half-reactions: Cu2+(aq) + 2e- --> Cu(s) Eo= 0.34V Ag+(aq) + e- --> Ag(s)...
Consider the 2 half-reactions: Cu2+(aq) + 2e- --> Cu(s) Eo= 0.34V Ag+(aq) + e- --> Ag(s) Eo= 0.8V If you increase the concentration of Cu2+(aq), which of the following would be true about the cell potential E? It would remain constant It would increase It would decrease This cannot be determined
Reaction Eo Ag+(aq)+ e-→ Ag(s) 0.80V Zn2+(aq)+ 2e-→Zn(s) -0.76V What would be the cathode reactant in...
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)
Consider a voltaic cell based on the half-cells: Ag+ (aq) + e - Ag(s) E* =...
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
9) A sol'n in an electrolytic cell contains the ions Cu2+, Fe2+ & Zn2+. If the voltage (initially...
9) A sol'n in an electrolytic cell contains the ions Cu2+, Fe2+ & Zn2+. If the voltage (initially very low) is turned up, in which order will the metals be plated out onto the cathode? Cu2+(aq)2e-Cu(s); E0.34V Fe"(aq) + 2e-→ Fe(s);E"--0.44V Zn2+(aq) + 2e-→ Zn(s): E。--0.76V 10) How long will it take to produce a sol'n of pH 2.00 by electrolysis of 500 mL of 0.100 M AgN03(aq) at 0.240 Amperes? Anode: 2H2O(l) → 4H-(aq) + O2(g) + 4e-, E°...
help with these please Consider the following half-reactions: Half-reaction Eo (V) F2(g)+ 2e 2F (aq) 2.870V...
help with these please
Consider the following half-reactions: Half-reaction Eo (V) F2(g)+ 2e 2F (aq) 2.870V Sn2 (aq) + 2e- Sn(s) 0.140V Cr3 (aq) + 3e° _ Cr(s)-0.740V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will F2(g) oxidize Cr(s) to Cr3 (aq)? (6) Which species can be oxidized by Sn2 (aq)? If none, leave box blank. Consider the following half-reactions:...
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 =...
5. Consider the following set of half reactions Ag (aq)Ag (s) Cu2(a)2 e- Cu (s) Ai (aq)3eAl (s) Eo0.7996 V E0.342 V Eo-1.6632 V i. Which pair of half reactions would make the battery with the largest E cell? i. Identify the cathode and the anode for this battery, and calculate the value of E cell. i. Write the overall redox reaction that would take place in the battery above.
An electrochemical cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Cu(s) and Cu2+(aq). What species are produced at the electrodes under standard conditions? E° = +0.80 V Agt(aq) + e- → Ag(s) Cu2+(aq) + 2 e- → Cu(s) E° = +0.34 V O Ag(s) is formed at the cathode, and Cu(s) is formed at the anode. Ag(s) is formed at the cathode, and Cu2+ (aq) is formed at the anode. Cu(S) is formed...
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
9) A sol'n in an electrolytic cell contains the ions Cu2+, Fe2+ & Zn2+. If the voltage (initially very low) is turned up, in which order will the metals be plated out onto the cathode? Cu2+(aq)2e-Cu(s); E0.34V Fe"(aq) + 2e-→ Fe(s);E"--0.44V Zn2+(aq) + 2e-→ Zn(s): E。--0.76V 10) How long will it take to produce a sol'n of pH 2.00 by electrolysis of 500 mL of 0.100 M AgN03(aq) at 0.240 Amperes? Anode: 2H2O(l) → 4H-(aq) + O2(g) + 4e-, E°...
help with these please
Consider the following half-reactions: Half-reaction Eo (V) F2(g)+ 2e 2F (aq) 2.870V Sn2 (aq) + 2e- Sn(s) 0.140V Cr3 (aq) + 3e° _ Cr(s)-0.740V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will F2(g) oxidize Cr(s) to Cr3 (aq)? (6) Which species can be oxidized by Sn2 (aq)? If none, leave box blank. Consider the following half-reactions:...
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