A certain half-reaction has a standard reduction potential-0red== +0.90 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell thatmust provide at least 0.70 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.ロ→ロ0Is there a minimum standard reductionpotential that the half-reaction used atthe anode of this cell can have?yes, there is a minimum.☐vredIf so, check the "yes" box and calculatethe minimum. Round your answer to 2decimal places. If there is no lowerlimit, check the "no" box.no minimumŚ ?0Is there a maximum standard reductionpotential that the half-reaction used atthe anode of this cell can have?yes, there is a maximum.OvredIf so, check the "yes" box and calculatethe maximum. Round your answer to 2decimal places. If there is no upperlimit, check the "no" box.no maximumEE==X

It is given that E°cell ≥ 0.70 E°cat = 0.90 V

A certain half-reaction has a standard reduction potential Ered=+0.90 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.70 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? O yes, there is a minimum. 0 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 anode of this cell can have? O yes, there a maximum. = Ov 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. Ono maximum red ローロ e 2.

A certain half-reaction has a standard reduction potential Ered=+0.90 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.70 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? O yes, there is a minimum. 0 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 anode of this cell can have? O yes, there a maximum. = Ov 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. Ono maximum red ローロ e 2.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Similar questions

A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M1.0 M tin(IV) ion and 1.0 M1.0 M tin(II) ion, and another inert platinum electrode in a solution containing 1.0 M1.0 M cerium(IV) ion and 1.0 M1.0 M cerium(III) ion, connected by a salt bridge. Calculate the standard potential for this cell at 25°C25°C. Standard reduction potentials can be found in the standard reduction potentials table.
Suppose that you want to construct a galvanic cell from nickel and cadmium for a chemistry project. You take all the precautions necessary to deal with a toxic heavy metal like cadmium, and you decide to use a 0.01 M solution of cadmium nitrate as one of the electrolytes. If you need a cell potential of 0.17 V for this system, what concentration of NiCl2 should you use? (For a follow-up web research project, compare this nickel-cadmium system with the one that is used in a commercial Ni-Cd battery.)
Weighing a copper atom in an electrolysis experiment. A standard experiment involves passing a current of several amperes through a copper sulfate solution (CuSO4) for a period of time and determining the mass of copper plated onto the cathode. If it is found that a current of 1.00 A flowing for 3600 s deposits 1.185 g of copper, find (a) the number of copper atoms deposited, (b) the weight of a copper atom, and (c) the molar mass of copper.
A voltaic cell is constructed at 25 °C from a half-cell in which a nickel rod is dipped into a solution of nickel (II) nitrate, and another half cell in which a chromium rod is dipped into a solution of chromium (III) nitrate. The two half-cells are connected by a salt bridge. Write the reduction half-reaction.
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A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of copper in a 1.0 M copper(I) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. E cell || = V
A galvanic (voltaic) cell contains a copper cathode immersed in a copper(I) chloride solution and a nickel anode immersed in a nickel(II) chloride solution. The two solutions are connected with a salt bridge. Write the balanced equation for the galvanic cell. Phases are optional. balanced equation: A current of 2.40 A is observed flowing through the cell for a period of 2.81 h. Calculate the amount of charge flowing through the circuit during this time. C Calculate the number of moles of electrons flowing through the circuit during this time. moles of clectrons: Calculate the mass change in grams of the copper and nickel electrodes. mass change of copper clectrodc: mass change of nickel electrode:
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