Can someone please help with question 9 1302 - 4.3 - + Analysis of Electroplating - Copy - Copy9 of 15I Review I Constants | Periodic TableWhen electricity (the flow of electrons) is passed through a solution, it causes an oxidation-reduction (redox) reactionto occur. If the solution contains a metal cation such as Ag+ , the flow of electrons will reduce the silver ion, causingsolid silver to plate onto the electrode. The amount of metal plated depends on the number of electrons passed. Thetotal charge of a mole of electrons is 96,485 coulombs (C) and1 ampere (A) = 1 coulomb/second (C/s)Part AWhat mass of Cu(s) is electroplated by running 23.5 A of current through a Cu+ (aq) solution for 4.00 h?Express your answer to three significant figures and include the appropriate units.?ValueUnitsSubmitRequest AnswerPart BHow many minutes will it take to electroplate 25.1 g of gold by running 5.00 A of current through a solution ofAu*(aq)?Express your answer to three significant figures and include the appropriate units.HÀValueUnitsSubmitRequest Answer

A) Given : Current passed = 23.5 A And time = 4.00 hr = 4.00 X 60 X 60 = 14400 s…

Part A What mass of Cu(s) is electroplated by running 23.5 A of current through a Cu?+ (aq) solution for 4.00 h? Express your answer to three significant figures and include the appropriate units. HẢ Value Units Submit Request Answer Part B How many minutes will it take to electroplate 25.1 g of gold by running 5.00 A of current through a solution of Au*(aq)? Express your answer to three significant figures and include the appropriate units.

Part A What mass of Cu(s) is electroplated by running 23.5 A of current through a Cu?+ (aq) solution for 4.00 h? Express your answer to three significant figures and include the appropriate units. HẢ Value Units Submit Request Answer Part B How many minutes will it take to electroplate 25.1 g of gold by running 5.00 A of current through a solution of Au*(aq)? Express your answer to three significant figures and include the appropriate units.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 57QRT

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4.112 A metallurgical firm wishes to dispose of 1300 gallons of waste sulfuric acid whose molarity is 1.37 M. Before disposal, it will be reacted with calcium hydroxide (slaked lime), which costs $0.23 per pound. (a) Write the balanced chemical equation for this process. (b) Determine the cost that the firm will incur from this use of slaked lime.
Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?
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Gold can be dissolved from gold-bearing rock by treating the rock with sodium cyanide in the presence of oxygen. 4 Au(s) + 8 NaCN(aq) + O2(g) + 2 H2O() 4 NaAu(CN)2(aq) + 4 NaOH(aq) (a) Name the oxidizing and reducing agents in this reaction. What has been oxidized, and what has been reduced? (b) If you have exactly one metric ton (1 metric ton = 1000 kg) of gold-bearing rock, what volume of 0.075 M NaCN, in liters, do you need to extract the gold if the rock is 0.019% gold?
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