metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5 in x 8.5 in x 0.0012 in. The gold plating must be 0.0020in thick. (a) How many kilograms of gold are produced. (b) How long will it take to plate the sheet from AuCN using a current of 7.00A?

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: How many seconds are required to deposit 0.274 grams of manganese metal from a solution that…

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Q: A current of 10.0 amperes flows for 2.00 hours through an electrolytic cell containing a molten salt…

A: According to the reaction given, we have  Xn+ (aq) + ne-→X (s) t=2 hours=7200 sec (since 1 hr =3600…

Q: A metallic object to be plated with copper is placed in a solution of CuSO.. What mass of copper…

A: Given,  Current, I = 0.22 amp  Time, t = 1.5 hours               = 5400 sec  Molar mass of Cu =…

Q: Determine the mass of nickel that shall be electroplated from a solution of nickel (II) chloride by…

A: Given  Current (i) = 0.25 amperes Time (t) = 10 hours  = (10×60×60) seconds  t = 36000 seconds  Mass…

Q: You have a 10.0 cm diameter sphere that you would like to have plated with gold metal. How long…

A: V_uncoated = (4/3)πr^3 = (4/3)π(5.00 cm)^3 = 523.33 cm^3 (diameter=10/2=5cm) Since the coating is…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

Q: 3. (a) Liquid NH3 is subjected to electrolysis. One of the half-reactions is 2 N3 N₂+6 e How many…

A: Given data:The given reaction is :a) How many faradays of electricity are required to produce 4.12 L…

Q: (b) A constant current was passed through a solution of AuCl; between gold (Au) electrodes. After a…

A: Given, Mass of gold deposited = 2.628g Time = 20min = 1200 second

Q: A thin circular-disk earring 4.00 cm in diameter is platedwith a coating of gold 0.25 mm thick from…

A: GIVEN: Diameter of earring =4.00cm Thickness of coating=0.25 mm Current(I) = 0.013 A d of gold =19.3…

Q: How many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a…

A: The amount of metal deposited on electrode is given by Faraday's first law of electrochemistry,…

Q: Copper is electroplated from CuSO4 solution. A constant current of 4.28 A is applied by an external…

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Q: In the electrolysis of a 200 mL metal experiment, 0.0434 grams of cathode is applied when a current…

A: Given: weight of metal(w) = 0.0434  Current(I) = 0.50 A  Time(t) = 5 min = 300 sec  Valency factor =…

Q: How many seconds are required to deposit 0.266 grams of cadmium metal from a solution that contains…

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Q: Determine the molar mass (amu) of Metal (M) if it took 1.04 minutes for a current of 1.22 A to plate…

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Q: 7) The voltage required to electrolyze certain solutions changes as the electrolysis proceeds…

A: Faraday's first electrolysis Law states that the quantity of reaction taking place in terms of mass…

Q: An electrolysis cell contains a solution of 0.10 M NiSO4. The anode and cathode are both strips of…

A: Electrolysis is spitting of chemical decomposition of ionic substances due to passage of electric…

Q: In a galvanic cell, one half-cell consists of a tin strip dipped into a 1.00 M solution of Sn(NO3)2.…

A: Given , Cell voltage = 0.595 V

Q: (a) Write the anode and cathode reactions and the overall reaction occurring in a lead storage…

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Q: How many seconds are required to deposit 0.218 grams of tin metal from a solution that contains Sn2+…

A: F = 96500 C mol-1 Current = charge/time

Q: ed through an aque- the yolume of Or

A: m = ( M • I • t ) / nF  m/M = ( I • t ) / nF  n = I • t / nF  Where, m = mass and M = molar mass and…

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

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Q: Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

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Q: A current of 9.22×104 A is passed through an electrolysis cell containing molten CaCl, for 10.9…

A: We will use relation of mass and gm equivalent

Q: Based on the cell potential measured for the cells Co(s) | Co²*(aq) || Cu²*(aq) | Cu(s) Fe(s) |…

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Q: Magnesium bars are connected electrically to underground iron pipes to serve as sacrificial…

A: Electrochemical cell is defined as the cell in which chemical energy is converted to electrical…

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: Determine the molar mass (amu) of Metal (M) if it took 2.85 minutes for a current of 1.1 A to plate…

A: Molar mass can be calculated as:-

Q: A current of 2.90 A was applied to an electrolytic cell containing molten CdCl2 for 54 minutes.…

A: We have to calculate the mass of cadmium metal deposited when current passed is 2.90 A for 54…

Q: In a certain electrolysis experiment involving Al" ions, 50.4 g of Al is recovered when a current of…

A: Given data : In a certain electrolysis experiment involves Al3+ ions  50.4 g of Al is recovered by…

Q: (a) How long (in hours) does it take to produce 454 g of copper from a solution containing Cu²*…

A: Given: The mass of copper to be produced from Cu2+ = 454 g We have to find the amount of energy (in…

Q: How many seconds are required to deposit 0.128 grams of magnesium metal from a solution that…

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Q: How long does it take to deposit a coating of gold 1.00 μm thick on a disk-shaped medallion 4.00 cm…

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Q: How many grams of copper metal will be deposited from a solution that contains Cu2+ ions if a…

A: Here we use the formula of metal deposited= ZIt , where Z is molecular weight, I= current, t= time…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.29 minutes for a current of 1.48 A to plate…

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Q: Molten CaCl₂ can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A: For CaCl2 , the given data is- Current(I) = 2.06A Mass of Ca = 29.3g Atomic mass of Ca = 40.078 g…

Q: How many seconds are required to deposit 0.136 grams of copper metal from a solution that contains…

A: Given, mass of Cu deposited = 0.136 g Current passed = 0.913 A 1 Faraday is the magnitude of charge…

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

A: Current = 5 A Voltage = 4.5 V Time = ? Volume = 215 mL = 0.215 L Molarity = 1.19 M

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…

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.