A thin circular-disk earring 4.00 cm in diameter is platedwith a coating of gold 0.25 mm thick from an Au³⁺ bath.(a) How many days does it take to deposit the gold on one sideof one earring if the current is 0.013 A (d of gold =19.3 g/cm³)?(b) How many days does it take to deposit the gold on both sidesof the pair of earrings?(c) If the price of gold is $320 per troy ounce (31.10 g), what is the total cost of the gold plating?

Q: 6b. How long does it take to deposit a coating of gold 1.00 picometers thick on a disk-shaped…

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Q: What mass of Mg is produced (in grams) when a constant current of 0.752 A is passed through an…

A: Given current (I) = 0.752 A time (t) = 14.2 hours molar mass = 24.31 g/mol electrons transfer  = 2

Q: 14H

A: Given data set: Molarity of K2Cr2O7 = 1.25 M Volume of K2Cr2O7 = 215 ml = 0.215 L Thus, Moles of…

Q: How many y seconds are required to deposit 0.216 grams of silver metal from a solution that contains…

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

A: Faraday’s first law - Faraday's first law of electrolysis describes that amount of substance…

Q: A voltaic cell is constructed with an Fe/ Fe²⁺ half-cell and an Mn/Mn²⁺ half-cell. The iron…

A: The two half cells in given cells are Fe/Fe2+ and Mn/Mn2+ of these manganese undergo oxidation and…

Q: How many grams of copper metal can be deposited from Cu2*(aq) when a current of 2.50 A is run for…

A: current =2.50 A Time = 1.90 hours  The calculation of the amount of charge is as follows: Charge =…

Q: How many minutes are required to deposit 2.28 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A: Faraday's Law of Electrolysis: According to this law during electrolysis, the amount of chemical…

Q: A voltaic cell is constructed with an Ag/Ag²⁺ half-cell and a Pb/Pb²⁺ half-cell. The silver…

A: a) The two half cells in given cells are Ag/Ag+ and Pb/Pb2+ of these lead undergo oxidation and…

Q: How many minutes are required to deposit 1.39 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A:

Q: How many grams of copper metal can be deposited from Cu2*(aq) when a current of 2.50 A is run for…

A:

Q: How many minutes are required to deposit 1.42 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A: Given:  W = 1.42 gm  I = 2.50 A  Mol. Wt. of Cr = 52  'n' factor of Cr = 3  Equivalent wt. of Cr =…

Q: 6) Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below.…

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Q: (a) One method to reduce the concentration of unwanted Fe3+(aq) in a                 solution of…

A: The half-reactions are oxidation or reduction reactions, which is useful in balancing redox…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cu2*(aq)…

A:

Q: A current of 5.99×104 A is passed through an electrolysis cell containing molten CaCl2 for 20.1…

A: Answers given as follows

Q: You want to design a galvanic cell using an iron (Fe) electrode as the cathode. Which of the…

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Q: Semimetallic silicon can be made by the electrolysis of molten SiO2. (a) What mass of Si is formed…

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Q: Brass, an alloy of copper and zinc, can be produced by si-multaneously electroplating the two metals…

A:

Q: 2+ If the anode of a galvanic cell is composed of Fe/Fc" (, which of the following should be used as…

A: Welcome to bartleby ! We have to tell which one of them is best for cathode cell so that voltage…

Q: 2+ A current of 3.40 A is passed through a solution containing Cu²+ (aq) for 30.0 minutes, with…

A:

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: a) 215 ml  ofb1.25  potassium  means (1.25/1000)×215 = 0.26 mol of potassium dichromate.   From the…

Q: 12) What mass of silver can be plated onto an object in 67 minutes at 8.70 A of current? Ag'(aq) + e…

A: Given ->  Time (t) = 67 minutes = 67 × 60 seconds= 4020 s  (1minute = 60 seconds)  Current (i) =…

Q: A constant electric current flows for 3.55 h through electrolytic cells connected in series. One…

A: According to the Faraday's  first law of electrolysis Deposition of an element  due to the flow of…

Q: (4) When a metal of molar mass 207 g mol" is deposited by electrolysis, a current of 0.06 A flowing…

A: Convert the unit of time: 1 min=60 s66 min=66 min×60 s1 min=3960 s

Q: How many grams of zinc metal will be deposited from a solution that contains Zn2* ions if a current…

A:

Q: galvanic cell is constructed in which a Pt | Fe2+ Fe3+ half-cell is connected to a Cd2+ | Cd…

A:

Q: How many minutes are required to deposit 1.48 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A: According to Faraday's law of electrolysis, the mass (m) of substance deposited at the electrode is…

Q: How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for…

A: Given, Current deposited = 2.50  Time = 2.95 h F = 96500 C/mol

Q: How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for…

A: By using Faraday law, we can find mass of Cu deposited at respective electrode.   The following…

Q: For the reaction below, (a)construct a galvanic cell. Label the parts and the flow of electrons.…

A: Ca(s) + Cd2+(aq)  --> Ca2+(aq) + Cd(s)

Q: How many seconds are required to deposit 0.145 grams of zinc metal from a solution that contains Zn*…

A: Answer :-  t = 447 (s) The time required to deposit 0.145 g of Zn metal from a Zn2+ solution when…

Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

A: According to electro-chemistry  W = zCt W= mass of Metal deposited in grams C= current  t = time in…

Q: What mass of each of the following substances can be produced in 1.2 h with a current of 11 A? (a)…

A: Current = 11 ATime = 1.2 h

Q: How many grams of iron metal are plated out when a constant current of 8.50 A is passed through…

A: We have 8.5 A of current, passed for 50 minutes, we have to calculate the mass of iron metal…

Q: A voltaic cell is constructed with a Cu/Cu²⁺ half-cell and an Ni/ Ni²⁺ half-cell. The nickel…

A: Given data: 1. The nickel electrode is -ve. As the -ve electrode in a voltaic cell is anode, the…

Q: what mass in grams of nickel could be elextroplated from a solution of Ni2+ by a current of 0.25…

A:

Q: (a) The standard reduction potential for X/X and Y/Y at 285 K are 0.52 V and 0.37 V respectively.…

A: Solution: In the given problem we have given reduction potential values and we have to represent the…

Q: How many grams of zinc metal will be deposited from a solution that contains Zn² ions if a current…

A:

Q: How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for…

A: As per the given information  current =2.50 A Time = 5.30 hours or  The calculation of amount of…

Q: How many minutes are required to deposit 2.73 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A: Given : I= 2.50 A F = 96500 C/mol Quantity of charged passed = I*t = 2.5*t = 2.5t 2.5t C deposits Cr…

Q: A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb2+ half-cell. The silver electrode…

A: Here we have to construct a voltaic cell with an Ag/Ag+ half cell and a Pb/Pb2+ half cell and write…

Q: A current of 8.46x1oʻ A is passed through an electrolysis cell containing molten KCi for 10.3 days.…

A: Given Current I = 8.46*104 A Time = 10.3 days Temperature = 273 K Pressure = 1 atm

Q: How many seconds are required to deposit 0.175 grams of cadmium metal from a solution that contains…

A:

Q: A current of 7.14×10“ A is passed through an electrolysis cell containing molten KCl for 13.9 days.…

A: Current I = 7.14 * 104 A Time t = 13.9 days  We need to find out how much potassium and chlorine is…

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.