Part A. How many seconds are required to deposit 0.123 grams of tin metal from a solution that contains Sn2+ ions, if a current of 1.09 A is applied? ____________s   Part B. Now, how many amperes are required to deposit 0.250 grams of copper metal in 876 seconds, from a solution that contains Cu2+ ions? ____________A

Q: Silver can be plated out of a solution containing Ag+ according to the half-reaction:Ag+(aq) +…

A: Given, Mass of silver = 12g I = 3.0A

Q: How many grams of gold will be plated out by a current of 0.35 A applied for 65 minutes from a…

A: Given reaction is  Au3+ (aq) +   3e-    →  Au (s) According to Faraday's law, equivalent weight of a…

Q: How many minutes would be required to electroplate 25.0 grams of chromium by passing a constant…

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Q: Cr2O7 2- (aq) + 14H+  6e- ---> Cr3+(aq) + 7H2O(l) Ered = 1.33V Cu2+(aq)  + 2e-  --> Cu(s) ?°red =…

A: For the given cell reaction the reduction potential of the electrodes is as follows: Cr2O7 2- (aq) +…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.21 minutes for a current of 1.24 A to plate…

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Q: Determine the molar mass (amu) of Metal (M) if it took 2.91 minutes for a current of 1.2 A to plate…

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Q: A zinc bar (atomic mass = 65.38 g/mol; ion charge = 2) is weighing 2.08 kg is attached to a buried…

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Q: A current of 5.18 A is passed through a Sn(NO,), solution for 1.70 h. How much tin is plated out of…

A: Please find your solution below :

Q: Which of the following species could offer cathodic protection for aluminum?   Standard Electrode…

A: Cathodic protection for aluminum, would preserve the metal by providing a highly active metal as an…

Q: Zinc plating (galvanizing) is an important means of corrosion protection. Although the process is…

A: The Faraday’s first law of electrolysis state that the mass of the substance  deposited at any…

Q: What current is needed to deposit 0.500 g of chromium metal from a solution of Cr3+ in a period of…

A: The formula for the calculation is W= Z x I x t Where W = amount of chromium deposited(0.500g)…

Q: A     constant current     of     0.800     A     is     used to deposit copper     at    the…

A: I = 0.8A t = 15.2min F = 96485 C Cu deposited at cathode. O2 deposited at anode. Mol. mass of Cu =…

Q: Calculate the voltages of the following voltaic cells under the conditions specified: a) Cd…

A: (a) The given cell reaction is : Cd2+(0.020 M)+Zn(s) →Zn2+(0.50 M) +Cd(s)

Q: current of 0.075A passes through a solution of silver nitrate for 10 minutes. How much silver is…

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Q: A current of 20.0 amps is applied to a Zn2+ solution. How many minutes will it take to reduce 15.0…

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Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.55 minutes for a current…

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Q: Consider an electrolytic cell with a steady current of 158 amperes which produces Als) (atomic mass…

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Q: Using a constant current of 6.9 A, a metal object is to be gold-plated by an electrolytic procedure…

A: Consider the given information is as follows; Current (I) = 6.9 A Time (t) = 9.8 min = 9.8×60=588…

Q: Sketch a detailed galvanic cell and label each of the specific species in the reaction (label each…

A: A question based on sketching galvanic cell, which is to be accomplished.

Q: Consider an electrolytic cell with a steady current of 169 amperes which produces Als) (atomic mass…

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Q: Ağ metal is oxidized to AgCI(s) on the surface of the Ag electrode in a 0.1 M HCI solution. At a…

A: The time 1 minutes is equal to 60 second. Total number of moles of electron transferred in the…

Q: [A4] Consider: Ag2S(ag) + Au(6) → 2Ag) + S2- + S2-(a0) + Au³+ (aq) (a) write out the reduction…

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Q: How many minutes does it take to plate 164.8g of chromium onto a car part using 16.75 A of current…

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Q: 15. How many minutes would a current of 20.0 amps need to run through a solution containing Au*3 to…

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Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.14 minutes for a current…

A: Answer :- Molar Mass = 144.52  ------------------------------------------------

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.39 minutes for a current…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.57 minutes for a current…

A: The molar mass can be find using Faraday law of electrolysis.   Faraday law state that mass of metal…

Q: v. Another electrolysis experiment is conducted using an Al³+ solution. Calculate the current…

A: The formula thats will be used here is as follows: Charge (Q) = Current (I) × Time (s) Unit of…

Q: Using a current of 4.75 A, how many minutes does it take to plate onto a sculpture 1.50 grams of Cu…

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Q: A current of 5.739 A is applied to an unknown metal nitrate solution, M(NO3)2, for 60.0 minutes. M2+…

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Q: 405−mL solution of NaCl was electrolyzed for 5.80 min. If the pH of the final solution was 12.23,…

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Q: Consider a galvanic cell below and calculate the concentration of Au*3 solution. The measured cell…

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Q: What current (in A) is required toplate out 1.22 g of nickel from a solution of Ni2+ in 1.0…

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Q: A 650.0 mL solution contains 1.0 M Ag+(aq) and 1.0 M Cu+(aq). A current of 7.50 amps was then…

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Q: estion 8 Copper is electroplated from a CuSO4 solution. A constant current of 4.57 A is applied by…

A: Given:: Mass of Cu = 1.198 g molar mass of Cu = 63.546 g mol-1 Current = 4.57 A Time (t) in minute =…

Q: What current in ampere will be required to produce 2.369 x10-3 kg of cu from CuS04 solution in one…

A: Provided time(t)= 1 hours Provided time(t)= 3600 second Provided Molar mass of Cu=63.5g/mol…

Q: How many grams of nickel would be electroplated by passing a constant current of 13.84 A through a…

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Q: Consider the cell described below. Al | Al3+ (1.00 M) || Pb²+ (1.00 M) | Pb Calculate the cell…

A: Consider the cell :  Al | Al3+(1.00 M) || Pb2+(1.00 M) | Pb  Changed concentration for Al = 0.46…

Q: 1.How many grams of NaCl is present on 5.0 mL of 1.0 % m/V NaCl solution?

A:

Q: 670.24 sec

A: Given data are as follows: Weight of silver deposited = 1.5 g Current passed = 2A

Q: A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each…

A:

Q: An unknown metal M is electrolyzed. It took 74.1 s for a current of 2.00A to plate out 0.107g of the…

A: Given,

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.91 minutes for a current…

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Q: A baby'sspoon with an area of 6.25 cm2 is plated with silver from AgN03 using a current of 2.00 A…

A: (a),

Q: MnO4– + Sn ---> MnO2 + Sn2+ a) What is the half reaction that takes place at the cathode? b) What…

A: Recall the given reaction       Mn7+O4- + Sn0 → Mn4+O2 + Sn2+ Recall values of standard electrode…

Q: How many minutes would a current of 20.0 amps need to run through a solution containing Au*3 to…

A: Amount of the current flow = 20A Mass of liberated substance = 10g Electron transfer per ion = 3

Q: A current of 0.44A is passed through a solution of ruthenium nitrate causing reduction of the metal…

A: