A galvanic cell is made up of one electrode consisting of a copper metal immersed in 0.00500 M Cu(NO3)2 and another electrode with a piece of silver metal that is immersed in an aqueous solution containing 0.235 M AgNO3. a) Identify which acts as the anode and the cathode in this cell. b) Write the galvanic cell notation. c) Calculate the cell potential.

1)A voltaic cell is constructed, based on the Zn/Sn2+ ion reaction. Zn + Sn2+ → Zn2+ + Sn The standard cell potential is 0.626 V.  Temperature is 298 K. What is the cell potential when [Zn2+]=0.7 M and [Sn2+]=1.3 M ?

A galvanic (voltaic) cell consists of an electrode composed of iron in a 1.0 M1.0 M iron(II) ion solution and another electrode composed of copper in a 1.0 M1.0 M copper(I) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C.25 °C. Refer to the list of standard reduction potentials.

A certain half-reaction has a standard reduction potential E=+0.21 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.00 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 anode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? Data O yes, there is a minimum. E red = v 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. O no minimum Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? O yes, there is naximum. Pred = Iv 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. no maximum By using the information…