A galvanic cell is built by connecting two half cells formed by silver and copper electrodes immersed in their respective solutions of 1 M AgNO3 and 1 M CuSO4. emf Cu2 + / Cu = 0.34 V, emf Ag + / Ag = 0.80 V a) Calculate the theoretical potential of the formed cell. b) Determine the amount of metal deposited on the cathode when 2.5 g of the anode is consumed. F = 96500 C. mol-1

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…

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction: 2Cr3+(aq)+3Ca(s)--->2Cr(s)+3Ca2+(aq) Suppose the cell is prepared with 1.96 M Cr3+ in one half-cell and 6.08 M Ca2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

An electrochemical cell is constructed by dipping a zinc rod in a solution of Zn(NO3)2(aq), dipping a cobalt rod in a solution of CoCl2(aq), and connecting them with a wire and a salt bridge. In the cell that is constructed, the metallic zinc is being oxidized. d. The standard cell potential for this electrochemical cell is 0.482 V and two moles of electrons are exchanged per mole of reaction. What is equilibrium constant, K, for the redox reaction described by this electrochemical cell at 298 K?

Consider the following electrochemical cell in which X is an unknown metal:       Pt (s) | Cl–(1 M) | Cl2 (1 atm) || X2+(1 M) | X (s)If the standard cell emf is 0.23 V, what is the standard reduction potential at 25○C for X2++ 2 e– → X (s)

The emf of a standard X-Y galvanic cell is -2.763V. If the standard half-cell emf for the oxidation of X at the anode is – 3.04V, what is the standard half-cell emf of Y if Y is the cathode?

The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn^2+(0.20 M)|| H+ (test solution)| H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for is –0.76 V. (Enter your answer to two significant figures.) pH =

A galvanic (voltaic) cell consists of an electrode composed of manganese in a 1.0 M manganese(II) ion solution and a second electrode composed of cobalt in a 1.0 M cobalt(II) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Use this list of standard reduction potentials. E: cell V

A certain half-reaction has a standard reduction potential Eed=+0.45 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.40 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. olo Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? yes, there is a minimum. E red Ov Ar 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. no minimum Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? E = Ov yes, there is a maximum. red 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

A galvanic cell was constructed with a nickel electrode that was dipped into 1.3 M NISO4 solution and a chromium electrode that was immersed into a solution containing Cr³+ at an unknown concentration. The potential of the cell was measured to be 0.564 V, with the chromium serving as the anode. The standard cell potential for this system was determined to be 0.487 V. What was the concentration of Cr³+ in the solution of unknown concentration? [Cr³+] = i M