A Pt wire is immersed in a solution containing V2+ and V3+ at equal activities of 0.01000. This half-cell is connected through a salt bridge to a Ag-AgBr half-cell in which aBr-= 0.100. The EMF of this galvanic cell is measured to be 0.385 V at 25 C and the electrode in the vanadium solution is the negative electrode. What is the standard electrode potential of the V2+-V3+ electrode? Write out the galvanic cell reaction.

The following half-cells are on the left and coupled with the standard hydrogen electrode on the right to form a galvanic Calculate the cell potential. If the cell were shorted, indicate whether the electrodes shown would act as an anode or a cathode. a. Cu Cu²+ (0.0567 M), (Cu²+/Cu = 0.337 V) V Potential = b. Cu | Cul (sat'd), KI (0.0939 M), (ECul/Cu = -0.185 V) Potential = V 3+ c. Pt | Fe³+ (0.160 M), Fe²+ (0.08340 M), (E Potential = V Fe³+/Fe²+ = = 0.771 V)

A certain naif-reaction has a standard reduction potential Ed-0.53 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.80 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no tower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the…

Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the voltage of a battery made from zinc in a 0.5M solution of Zn2+ and a metal X in a 1 M X2+ solution using the table of reduction potentials and Eq. 6 at 25 degrees C. Answer with the unit V, to two decimal places. The standard reduction potential of X is -0.19 volts. Your Answer:

John makes a galvanic cell with the half-reactions Mt3+(aq) + 3e1- -->Mt(s), and R2+(aq) + 2e1- --> R(s), with standard reduction potentials of 1.09 V and 0.34 V respectively. Would the value of the Gibbs free energy decrease, increase, or remain the same, if he changes the concentrations in the galvanic cell to 0.15 M Mt3+, and 0.45 M R2+?

Three voltaic cells can be constructed from solutions Pb(NO3)2(aq) and the corresponding metal electrodes. of Cuso (aq), ZnSOa(aq), and Reaction E Zn?daa) + 2e s zn(s) -0,7626V Pbaas + 2e 5 Pb (S) - 0.1251 V Calculate the standard cell potential for each voltaic cell combination. For a spontaneous reaction, E'cell must be positive when E'anode is subtracted from E'cathode. Use the standard potentlals from p. 119 for calculations. 1. * 2e- ニ Cucs) 0. 340 V Agčaa) e- 5 Ag(s) 0.7991 2. Identify which metal electrode serves as the cathode and which metal electrode serves as the anode. Tabulate the results from questions 1 and 2: E'cell Cell Anode Cathode Cu/Zn Cu/Pb Pb/Zn 3.a. Using the Nernst Equation, calculate the expected voltage (Etheo) for a cell which consists of 0.0300 M Pb(NOs)2(aq) and 0.0400 M CuSO (aq). b. Glve the conventional cell notation for this cell, assuming a salt bridge separates the two half- cells.

A voltaic cell consists of an Al/Al3+ half-cell and a Fe2+/Fe3+ half-cell.  The standard reduction potential for Al3+ is −1.66V and for Fe3+ is 0.77 V.  Calculate Ecell at 25 ºC when the concentration of [Al3+] = 9.51 x 10-4 M , [Fe3+]= 6.24 x 10-3 M, and [Fe2+]= 5.74 x 10-5 M

Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the anode of this cell. Note: write the half reaction as it would actually occur at the anode. Oyes, there is a minimum. no minimum yes, there is a maximum. no maximum 0 E 0V red 0 E red = = ☐v

For the following electrochemical cell: Mn(s)|Mn2+(aq)(.215M)||Cr3+(aq)(.113M), Cr2+(aq)(.301M)|Pt(s) Determine the cell potential for this electrochemical cell by first calculating the standard cell potential and then by using the Nernst equation.