You have a 5.00 cm diameter sphere that you would like to have plated with copper metal. How long will it take toelectroplate a 40.0 micron thick coating onto the sphere using Cu+2 and a current of 3.00 amps? The density of copper is8.94 g/cm³. 1 micron = 1.00×10-4 cm.[hint: Calculate the difference in volume of the coated and uncoated spheres and then use the density information todetermine your answer.]R

This answer is given below.Explanation:

Answered: You have a 5.00 cm diameter sphere that…

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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You pass a 2.5 amp current through an aqueous solution of aluminum nitrate for 5 hours. How many moles of solid aluminum metal would be formed? Report your answer in units of moles rounded to the nearest thousandth.
A certain metal M forms a soluble nitrate salt MNO33 . Suppose the left half cell of a galvanic cell apparatus is filled with a 5.00M solution of MNO33 and the right half cell with a 25.0mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0°C. What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode.Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
A constant current of 0.800 A was used to deposit copper at the cathode and oxygen at the anode of an electrolytic cell. Calculate the mass of each product that was formed in 15.2 min, assuming that no other redox reactions occur.
A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M chromium(III) ion and 1.0 M chromium(II) ion, and another inert platinum electrode in a solution containing 1.0 M cobalt(III) ion and 1.0 M cobalt(II) ion, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Standard reduction potentials can be found in the standard reduction potentials table. V. %3D 'cell
red A certain half-reaction has a standard reduction potential E = +0.16 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.30 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 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…
A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your teacher asks you to identify the cathode of the solution with the given information. The anode metal is lustrous and grey in color, so you narrow it down to silver and zinc. The voltmeter reading shows that the cell potential is 0.50 V. The copper (II) sulfate solution was indicated to have a concentration of 0.10 M. Reduction Half-Reaction Standard Reduction Potential (V) Ag+(ag) +e-→ Ag(s) +0.80 Cu2+(ag) +2e-→ Cu(s) +0.34 Zn2+(ag) +2e- → Zn(s) -0.76 Write the proper cell notation (with phases and concentrations) for the galvanic cell.
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Cu²+ (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ 2+ Suppose the cell is prepared with 1.56 M Cu in one half-cell and 6.31 M Zn Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 x10 •□ μ 0|0 Ś in the other.
A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell apparatus is filled with a 15.0 mM solution of MNO3 and the right half cell with a 3.00 M solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 30.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. O left 0 right x10 X
A non-standard state galvanic cell is constructed at 25.00°C as described here. The Fe(s) anode is immersed in a 0.040 M Fe(NO3)2 solution. The Cu(s) cathode is immersed in a 0.0060 M Cu(NO3)2. The circuit is completed with a salt bridge containing 1.0 M KNO3. The standard Fe/Fe2+ reduction potential is –0.44 V. The standard Cu/Cu2+ reduction potential is +0.34 V. Calculate the non-standard-state cell potential for this galvanic cell and determine if the reaction described is spontaneous under these conditions.
the Faraday constant. Suppose that after the electroplating was complete, you wiped the cathode copper strip very harshly with a tissue wipe (wiping off some of the electroplated copper off the strip) How would this specifically affect your calculated value of the Faraday constant?
. Consider the oxidation-reduction reaction Mg (s) + Cu2+ (aq) → Mg2+ (aq) + Cu (s) Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?
How long does it take to deposit a coating of gold 1.00 μm thick on a disk-shaped medallion 4.00 cm in diameter and 2.00 mm thick at constant current of 84 A? The density of gold is 19.3 g/cm3 and the gold is from an Au(III) solution.

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