Calculated Nonstandard Cell Potentials Ag+(0.010 M)|Ag(s) and Cu2+1Cu(s) 0.44
Part C. Effect of Concentration on Cell Potentials • Ecall for the Cu(s). Cu2+||Ag*, Ag(s) system: 0.450 V 0,851 v • Ecate for the Cu(s). Cu2+||Ag, Ag(s) system after the addition of 6M NH: • Write the balanced redox reaction for the entire cell: • • How many electrons are transferred? Use the Nernst Equation (given below) to calculate the concentration of Cu left in the solution Een = Ecen (0:0257) in (1960 [Cu2+] =
Calculate the cell potential for the reaction below when the concentrations of ions are: [Ag+ ] = 0.010 M and [Cu2+] = 0.750 M, at 25 °C. Cu(s) + 2Ag+ (aq) --> Cu2+(aq) + 2Ag(s) Given the standard reduction potentials: Cu2+(aq) + 2e– → Cu(s) Eϴ = 0.34 V Ag+ (aq) + e– → Ag(s) Eϴ = 0.80 V (A) 0.35 V (B) 0.44 V (C) 0.46 V (D) 0.48 V (E) 0.57 V
An Ag-Cd electrochemical cell is written as Cd (s) CdCl2 (0.010 M) || AgCl (s) CI- (0.50 M) | Ag E°Cd2+/Ca = 0.403 V and EºACIJAg = 0.222 V 1. Write the half-cell reactions at anode and at cathode. 2. Which is oxidant and which is reductant? 3. Calculate the half-cell potentials at both anode and cathode. 4. Calculate the cell potential. 5. Write the whole-cell reaction. 6. Calculate the equilibrium constant for the whole-cell reaction. For the half –...
For the following electrochemical cell: Cu(s) | Cu2+ (0.0179 M) || Ag+ (2.9 M) | Ag(s) Find the following at 25˚C: a. Net cell equation: b. E˚cell = c. E cell = d. ∆G˚rxn = e. ∆Grxn = f. Is this reaction spontaneous as written?:
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown in Table 5-1. (Note: for the iron solutions the Nernst equation must be used) Pb(s) | Pb(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) Cu(s) Zn(s) | Zn(NO3)2(0.1M) || Cu(NO3)2 (0.1M) Cu(s) Cds) | Ca(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) | Cu(s) Cu() Cu(NO3)2(0.1M) Il Fe (0.1M/Fe? (0.1M graphite Pb(s) Pb(NO3)2(0.1M) Il Fe3(aq) (0.1M)/ Fe2(aq) (0.1MI graphite(s) Zns | Zn(NO3)2 (0.1M) || Pb(NO3)2 (0.1M) | Pb(s) Cdis Ca(NO3)2...
Compare the potentials between the Ag/Ag+ and Cu/Cu2+ half cells before and after adding excess NH3 to the Cu/Cu2+ half cell. Did the potential increase or decrease? Explain the result in terms of the Nernst equation.
Identify the complete redox reaction for a CulCu2+||Ag+Ag cell. A. Cu(s) + Ag(s) Cu2+ (aq) + Ag+ (aq) B. Cu(s) + Ag+ (aq) + Cu2+ (aq) + Ag(s) c. Cu(s) + 2 Ag+ (aq) (aq) + 2 Ag(s) D. Cu²+ (aq) + 2 Ag(s) + Cu(s) + 2 Ag+ (aq) → Cu2+
Question 2 Consider a galvanic cell with the following cell notation: Cu(s)|Cu2+(0.0200 M) || Ag+ (0.0200 M)|Ag(s) a) Calculate the electrode potential at the cathode (Ecathode) b) Calculate the electrode potential at the anode (Eanode) c) Calculate the cell potential (Ecell)
During part B of your lab, you measured electrochemical cell potentials with a Cu2+/Cu couple as the anode. Predict the results you would observe if Ag+/Ag were the anode. half-cell predicted potential difference in V Cu2+/Cu Ag+/Ag Pb2+/Pb Zn2+/Zn
During part B of your lab, you measured electrochemical cell potentials with a Cu2+/Cu couple as the anode. Predict the results you would observe if Ag+/Ag were the anode. half-cell predicted potential difference in V Cu2+/Cu Ag+/Ag Pb2+/Pb Zn2+/Zn