(a)
Interpretation : The half reaction for given process needs to be determined.
Concept Introduction : Electroplating process involves an
(b)
Interpretation : If the ring act as anode or cathode needs to be determined.
Concept Introduction : Electroplating process involves an electrochemical reaction in which gold or silver is coated over other metal substances. Here when electricity is passed, the silver or gold ions discharge over other metal substance due to difference in their electrode potential.
(c)
Interpretation : The reason for need of energy to gold plate the ring needs to the explained.
Concept Introduction : Electroplating process involves an electrochemical reaction in which gold or silver is coated over other metal substances. Here, when electricity is passed, the silver or gold ions discharge over other metal substance due to difference in their electrode potential.
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Pearson eText Basic Chemistry -- Instant Access (Pearson+)
- The commercial production of magnesium is accomplished by electrolysis of molten MgCl2. (a) Why is electrolysis of an aqueous solution of MgCl2 not used in this process? (b) Write the anode and cathode half-reaction in the electrolysis of molten MgCl2.arrow_forwardA voltaic cell can be built using the reaction between Al metal and O2 from the air. If the Al anode of this cell consists of 84 g of aluminum, how many hours can the cell produce 1.0 A of electricity, assuming an unlimited supply of O2?arrow_forwardAn aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?arrow_forward
- A silver oxidezinc cell maintains a fairly constant voltage during discharge (1.60 V). The button form of this cell is used in watches, hearing aids, and other electronic devices. The half-reactions are Zn(s)+2OH(aq)Zn(OH)2(s)+2eAg2O(s)+H2O(l)+2e2Ag(s)+2OH(aq) Identify the anode and the cathode reactions. What is the overall reaction in the voltaic cell?arrow_forwardChlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode reaction is 2Cl(aq)Cl2(g)+2e How long will it take to produce 2.00 kg of chlorine if the current is 5.00 102 A?arrow_forwardA factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this?arrow_forward
- When molten lithium chloride, LiCl, is electrolyzed, lithium metal is liberated at the cathode. How many grams of lithium are liberated when 2.00 103 C of charge passes through the cell?arrow_forwardConsider the following cell running under standard conditions: Fe(s)Fe2+(aq)Al3+(aq)Al(s) a Is this a voltaic cell? b Which species is being reduced during the chemical reaction? c Which species is the oxidizing agent? d What happens to the concentration of Fe3+(aq) as the reaction proceeds? e How does the mass of Al(s) change as the reaction proceeds?arrow_forwardThe metallurgy of aluminum involves electrolysis of Al2O3 dissolved in molten cryolite (Na3AlF6) at about 950 C. Aluminum metal is produced at the cathode. Predict the anode product and write equations for the reactions occurring at both electrodes.arrow_forward
- An electrolysis cell for aluminum production operates at 5.0 V and a current of 1.0105 A. Calculate the number of kilowatt-hours of energy required to produce 1 metric ton ( 1.0103 kg) of aluminum. ( 1kWh=3.6106 J and 1J=1 C V.)arrow_forwardA voltaic cell is constructed from the following half-cells: a chromium electrode in chromium(III) sulfate solution and a lead electrode in lead(II) sulfate solution. The half-reactions are Cr(s)Cr3(aq)+3ePb2+(aq)+2ePb(s) Sketch the cell, labeling the anode and cathode (and the electrode reactions), and show the direction of electron flow and the movement of cations.arrow_forwardHalf-cells were made from a nickel rod dipping in a nickel sulfate solution and a silver rod dipping in a silver nitrate solution. The half-reactions in a voltaic cell using these half-cells were Ag+(aq)+eAg(s)Ni(s)Ni2+(aq)+2e Sketch the cell and label the anode and cathode, showing the corresponding electrode reactions. Give the direction of electron flow and the movement of cations.arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning