What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for 181 minutes using a constant current of 12.0 amperes?   a. 0.187 g b. 0.390 g c. 210.7 g d. 23.4 g e. 35.1 g

Q: A molten sample of CuCl2 is electrolyzed for 2.0 days at a current of 15.0 amps. How many grams of…

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Q: How many grams of Ca metal are produced by the electrolysis of molten CaBr2 using a current of 30.0…

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Q: A solution of a metal ion M 3+(aq) is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19…

A: The given data contains,       current =5 A      time =10 min60s1 min=600s

Q: Electrolysis of a molten salt with the formula MCl, using a current of 3.86 amp for 16.2 min,…

A: Record the given data, The given current (A) is 3.86 amp The given time in s is 16.2 x 60 = 972 s

Q: Consider an electrolytic cell where silver metal is plated (reduced) from an  aqueous silver nitrate…

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Q: Current is passed through a cell where the half-reaction that occurs at the cathode is 5e + MnO4 +…

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Q: 3. A factory wants to produce 1.0 x 103 kg Barium from the electrolysis of molten barium chloride.…

A: The given values are: m=1.0×103 kg=1.0×106 gt=4.0 h=4.0 ×3600 s The electrolysis step to form barium…

Q: An electrolysis cell that deposits gold (from Au ^+3 (aq)) operates for 11.0 minutes at a current of…

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Q: How long must a current of 5 amperes (A) be maintained to electroplate 60 g of calcium from the…

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Q: An aqueous Cu+2 solution is electrolyzed for 45 minutes. A 3.2 ampre current is used. What mass of…

A: Electrochemistry is the branch of chemistry that deals with the chemical processes that cause…

Q: 22). The electrolysis of a copper sulfate solution to get copper metal is carried out using a…

A: The chemical equation may be written as: Formula used: m = mass of Cu that deposits M = molar mass…

Q: 4. Calculate the quantity indicated for each of the following electrolysis. a. The mass of Žn…

A: Electrolysis is the process of using electric current to carry out a chemical reaction. This…

Q: 1. In an electrolysis of a solution containing Ni2+ (aq), metallic Ni(s) deposits on the cathode.…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: A current of 5.25 A is passed through an aqueous solution of copper(II) nitrate for 71.0 min. How…

A: An swer:- this question is answered by using the simple concept of calculation of mass of a metal…

Q: An electroplating solution contains vanadium (50.9415 g/mol), which is a metallic element that can…

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Q: Calculate the quantity indicated for each of the following electrolysis. a. The mass of Zn deposited…

A: The mass of zinc can be calculated by using Faraday's law of electrolysis.

Q: What mass of platinum could be plated on an electrode from the electrolysis of a Pt4+ (aq) solution…

A: The given data contains, Current =0.500 ATime =55 smolar mass ofPt=55 g/mol Charge =+4

Q: A solution of Mno is electrolytically reduced to Mn3+. A current of 7.79 A is passed through the…

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Q: How many grams of Ca metal are produced by the electrolysis of molten CaBr2 using a current of 30.0…

A: Given,  Current (I) = 30.0 amp Time (t) = 8.0 hours = 8.0 × 60 × 60 sec = 28800 sec Mass (in grams)…

Q: A solution containing vanadium (chemical symbol V) in an unknown oxcidation state was electrolyzed…

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Q: A solution of a metal ion Mag is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19 g of…

A: a.

Q: Gold (atomic mass = 197.0) is plated from a solution of chloroauric acid, HAuCl4; it deposits on the…

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Q: 1. Fischl, a scientist from Mondstadt specializing in electrochemistry, performed an electrolytic…

A: Given: The mass of metal deposited = 9.701 g. The current passed, (i) = 1.500 A. The time of passage…

Q: A steady current of 5 A  is maintained for 120 seconds in CuSO4 solution. How much Cu is deposited…

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Q: What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr,(SO)3 for 149…

A: From Faradays First law of electrolysis,  the amount of the substance deposited(W) at the given…

Q: Gold (atomic mass = 197.0) is plated from a solution of chloroauric acid, HAuCl4; it deposits on the…

A:

Q: A cell is constructed by immersing a strip of silver in 0.10 M AgNO 3 solution and a strip of lead…

A: Given: Cell prepared by AgNO3/Ag and Pb(NO3)2/Pb halves. And the concentration of Ag+ (from AgNO3 )…

Q: What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for 160…

A: Time = 160 minutes  Current = 12.0 ampere  Mass of chromium deposited during electrolysis = ?

Q: 8. An electrochemical cell is constructed with a zinc electrode immersed in a 1.0 M ZnCl₂ solution…

A: Determination of standard electrode potential for the given electrochemical cell: Zn2++ 2e-→Zn…

Q: current of 3.55 A is passed through a Cu(NO3)2 solution for 1.90 h. How much copper is plated out of…

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Q: A factory wants to produce 1.0 x 10³ kg Barium from the electrolysis of molten barium chloride. What…

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Q: One half-cell in a voltaic cell is constructed from a copper wire dipped into 0.40 M solution of…

A: First calculate the standard cell potential (E°cell) :

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A:

Q: A galvanic (voltaic) cell contains a copper cathode immersed in a copper(II) chloride solution and a…

A: In this question, we have to find out the correct answer of given problem by the help of the…

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.