A voltaic cell is based on the following half reactions at 25°C: Ag + e- →...
A voltaic cell is based on the following half reactions at 25 ⁰C: Ag + + e- à Ag E⁰ = 0.8V H2O2 + 2H+ + 2e- à 2H2O E⁰ = 1.78V Predict whether E cell is larger or smaller than E⁰ cell for the following cases. Explain your answers. (a) [Ag +] = 1.0 M, [H2O2] = 2.0 M, [H+] = 2.0 M (b) [Ag +] = 2.0 M, [H2O2] = 1.0 M, [H+] = 1.0 x 10-7 M
3. Calculate the cell potential for the voltaic cell based on the following half reactions at T = 25°C: Cr3+(aq) + 3e Cr(s) E° = -0.74 V TiO2(aq) + 2H(aq) + 1e → Ti+(aq) + H2O(1) E° = + 0.10 V Where, [Cr3+] = 1.0 x 104 M, [TiO2+] = 1.0 x 10-1M, [H+] = 1.0 M, [Ti$+] = 5.0 x 10-2 M.
Calculate the E of the cell based on the following half reactions: VO2+ (aq) + 2H+ (aq) + e- ----> VO2+ (aq) + H2O (l) Zn (s) --->Zn2+ (aq) + 2e- Under the following condition: T = 25°C [VO2+] = 2.0 M [H+] = 0.5 M [VO2+] = 1.0 x 10-2 M [Zn2+] = 0.10 M
1. A galvanic cell is based on the following half-reactions at 281 K: Agt + e + Ag E° = 0.803 V H2O2 (aq) + 2H+ + 2 e + 2 H20 E° = 1.78 V What will the potential of this cell be when [Ag+] = 0.501 M, [H+] = 0.00365 M, and [H2O2] = 0.867 M? Enon
4. The following balanced redox reaction occurs in voltaic cell at 25°C H2 (g) + 2Ag+ (aq) → 2H* (aq) + 2 Ag (s) 2H+ + 2e → H2 (g) EⓇ = 0.00V Ag (aq) + le → Ag(s) E = +0.80V a. Write the two half-reactions (oxidation and reduction) occurring in the cell. Clearly indicate which reaction shows oxidation and which shows reduction. Clearly indicate which reaction occurs at the anode and which reaction occurs at the cathode. (4...
A voltaic cell is based on the following two half-reactions: Cd2 (ag) +2e-> Cd (s) Sn2(aq)+ 2e Sn (s) Calculate the standard cell potential. Use the date from the attached table.SRP2.docx Oa 0.13 Ob 042 Oc.027 Od-0.27
Please show all work step by step and final answer. Reactions at Electrodes during Electrolysis Answer the following questions by selecting the appropriate half-reaction. Assume that in each case the experiment is performed in an electrolysis cell having electrodes made of non-reacting material. Which half-reaction will take place at the anode during the electrolysis of 1.0 M H2O2 solution containing 1.0 M H2SO4? O 02 + 4H+ + 4e - 2H20 H202 0 2 + 2H+ + 2e H2O2 +...
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.
I want to know the right way to do this and also the correct answer. Please help Reactions at Electrodes during Electrolysis Answer the following questions by selecting the appropriate half-reaction. Assume that in each case the experiment is performed in an electrolysis cell having electrodes made of non-reacting material. which half-reaction will take place at the anode during the electrolysis of 1.0 M AgNO3? 2H20 + 2 H2 + 20H Ag+ + e Ag 2H20 02 + 4H+ +...
What is the anode of the voltaic cell made by the combination of following half reactions? Reaction Standard Reduction Potential Zn2+ + 2e– → Zn E0 = –0.76 V Ag+ + e– → Ag E0 = +0.80 V Question options: a. Zn2+(aq) b. Ag+(aq) c. Ag(s) d. Zn(s)