What potential would you expect for the cell ZnlZn2+ (0.10 M) II Cu2+(0.10 M)|Cu? Show your...
calculate the cell potential of this reaction. Cu|Cu2+ (0.0100M)||Cu2+ (0.1M)|Cu . The half-cell reaction is Cu2+(aq) + 2e- --> Cu(s) with standard potential Eo is 0.3419V
What is the cell potential of a cell containing: A Cu electrode in 1.0M Cu2+ A Pt electrode in a solution of 1.0M Fe2+ and 1.0M Fe3+. A salt bridge
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
Consider the cell. Cu ∣ Cu2+ (0.00534 M)∣∣ Pb2+ (0.00735 M) ∣∣ Pb Calculate the half‑cell reduction potential at 298 K at the cathode. ? cu2+/cu=+0.34V ?cathode=......V Calculate the half‑cell reduction potential at 298 K at the anode. ? pb2+/pb=-0.13V ?anode=....V What is the initial potential needed to provide a current of 0.0800A if the resistance of the cell is 4.13Ω? Assume that ?=298 K. ?applied=......V
What is the potential of a cell made up of Zn/Zn2+ and Cu/Cu2+ half-cells at 25°C if [Zn²+1 -1.00 Mand (Cu2+] = 0.05 M?
A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 oC. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.370 V? Cu2+(ag) + Pb(s) → Cu(s) + Pb2+(ag) Hint: [Pb2+] + [Cu2+] = (1.5M + 0.05M) = 1.55 M total Hint: the standard potential of Pb2+ + 2e- → Pb(s) is -0.130 and the standard potential...
Effect of Temperature on Cell Potential Cell designation: E (measured) Temperature (°C) PbPb2+ || Cu2+ Cu; 0.455 Temperature (K) AG (calculated) 0.497 295 0.512 Sn Sn2+ || Cult | Cu; 0.548 0.554 279 295 0.566 343 Y AS determined from the slope of a plot of AG versus T AS Pb Cur AS Sn|Cu = AH° Pb | Cu=- AHSn Cu=- AHº calculated at 298 K (show calculations) from AG = AH-TAS AH = AG+TAS
If a platinum indicator electrode is used to measure [Cu^22^++] (standard reduction potential of Cu^22^++ is 0.337 V), and [Cu^22^++] = 0.0053 M, what is the cell potential (V) if the reference electrode is SCE and the measurement is taken at 298 K? Indicator Electrode--Quantification (Homework) Homework Unanswered If a platinum indicator electrode is used to measure [Cu2+] (standard reduction potential of Cu +is 0.337 V), and [Cu2+ o.0053 M, what is the cell potential (V) if the reference electrode...
A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 °C. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.370 V? Cu2+ (aq) + Pb(s) + Cu(s) + Pb2+ (aq) Hint: [Pb2+] + [Cu2+] = (1.5M + 0.05M) = 1.55 M total Hint: the standard potential of Pb2+ + 2e → Pb(s) is -0.130 and the...