What mass of chromium could be deposited from a solution of Cr3+ (aq) using a current of 10.0 A for 180 minutes? (Mc = 52.00 g/mol) А. 2.16 g В. 6.47 g С. 19.4 g D. 58.2 g

Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A: Ga3+ + 3e– ----> Ga(s)   Charge  = Current × time (s) = 0.830 A × (30.0 × 60 ) s = 1494 C

Q: How long will it take for a uniform current of 6.00 A to deposit 78.0 g gold (197.0 g/mol) from a…

A:

Q: How many minutes will it take to plate out 40 g of Ni from a solution of NISO4 using a current of…

A:

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

A: The Faraday's 1st law of electrolysis is one of the most important law which explains the…

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

A: The amount of substance deposited is directly proportional to the applied charge. Then the total…

Q: How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through…

A: Faraday's Law: It can be defined as by saying that the amount of substance produced at each…

Q: 4. A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5 in x 8.5 in x…

A: Given current = 7 A standard value  density of gold = 19.3 g/cm3

Q: How long must a current of 20.0 amps be applied to a solution of CrCl3 to produce 175 g of Cr (s)…

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: A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5in x 8.5in x…

A: first we have to find the volume,volume=length ×width×heightthen we know,density=massvolumeby…

Q: How many grams of Au would be deposited from an aqueous solution of Au 3+ with a current of 2.213 A…

A: Given, Molecular mass of Au = 196.96 u Current = 2.213 A time = 480 minutes = 28,800 sec

Q: An aqueous solution of copper (II) nitrate was electrolyzed using a current of 1.5 A for 60 minutes…

A: Given that -  Current used for copper (II) nitrate Electrolysis = 1.5 A  Time = 60 minutes = 60×60…

Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A:

Q: What mass of Ni(s) may be deposited from an aqueous NiCl2 solution if a current of 2.50 A is applied…

A: Reaction occuring  Ni+2 (aq) + e-  --------> Ni(s)

Q: Thorium, Th, is an actinide metal that can be used as a contact explosive much solid thorium could…

A: Given, Current is passed through Th4+ solution is ---- 0.51A Time is ---- 3hours How much thorium is…

Q: What is the efficiency of an electrolytic cell that produces 20.0 g of elemental chromium from a…

A: Efficiency of an electrolytic cell means its current efficiency. The current efficiency is a ratio…

Q: How long will it take to deposit 1.5 g of Cu on a metal when a current of 5 A is applied to a CuSO4…

A: Given- Amount of copper = 1.5 gMetal of interest = CuCurrent = 5 A To find- Time required

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

A: Mass of cobalt is calculated as:-

Q: current of 70.9 A is applied to a 0.123 mol L-1 solution of Pt2+ how many seconds would it take to…

A: Here we know nF of charge is required to produce 1 mole of Pt (s) as the products. So we do 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: Given:: Mass of Cu = ? molar mass of Cu = 63.546 g mol-1 Current = 2.50 A Time (t) = 2.45 h = 2.45 ×…

Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A:

Q: 4. A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5 in x 8.5 in x…

A: Given: The dimension of thin sheet = 1.5 in x 8.5 in x 0.0012 in The thickness of the sheet = 0.0020…

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: A metal was galvanized with zinc using a solution of zinc nitrate, Zn(NO3)2. How much time was…

A: Answer :  We have to calculate time to plate zinc on the metal . Using Faraday laws of electrolysis…

Q: How many hours are required to produce 5.00 g of chromium metal from an acidic solution of potassium…

A:

Q: (7.15a) What mass of copper is plated out in the electrolysis of CuSO4, in the same time that it…

A:

Q: How many grams of chromium metal will be deposited from a solution that contains Cr3+ ions if a…

A:

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

A:

Q: How many minutes would it take to plate 12g of silver from an aqueous Ag(l) solution using a current…

A:

Q: What mass of Ni2+Ni2+ is produced in solution by passing a current of 67.0 AA for a period of 14.0…

A: Electrochemical cell

Q: A current of 0.500 A flows through a cell containing Cd(II) for 10.0 minutes. Calculate the maximum…

A: Converting time from minute to second 10 min = 10 X 60 = 600 s charge = current X time = 0.500 A X…

Q: How much time is needed for a 1.00 g Ag to be deposited by electrolysis of a AgNO3 solution using a…

A:

Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A: Given information, Current = 0.490 A Time = 50.0 min = 3000 s

Q: What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for 181…

A: Given data: The time taken for the electrolysis of Cr2(SO4)3 is t=180 min. The current produced is…

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A:

Q: How much time is needed for a 1.50 g Ag to be deposited by electrolysis of a AGNO3 solution using a…

A: Correct Option :   892 s

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A:

Q: How much silver was there in the solution if all the silver was removed as Ag metal by electrolysis…

A: Given, Time (t) = 0.60 hr = 2160 s Current (I) = 1.00 mA = 1.00 × 10-3 A Amount (in grams) of silver…

Q: How much time is needed for a 1.00 g Ag to be deposited by electrolysis of a AgNO solution using a…

A: The mass of a substance deposited or liberated at any electrode is directly proportional to the…

Q: how many minutes are required to plate 10.0g of nickel metal from a solution of NiSO4, if the…

A:

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: How long will it take to deposit 1.5 g of Ag on a metal when a current of 2 A is applied to Ag+…

A: In electrolytic cells, electric energy is converted into chemical energy to run a chemical reaction.…

Q: In one application, a 0.010-mm layer of chromium must be deposited on a part with a total surface…

A: If you are not given which can be found so that I am answering the volume of Cr.

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

A: According to Faradey’s first law of electrolysis, the amount of substance liberated or deposited (m)…

Q: How much time (in s) is needed to deposit 0.0125 g of chromium from a solution of Cro+ with a…

A: Given Weight = 0.0125 Current = 1.5 A F = 96500 A-s/mol e- Molar mass of chromium = 52 g

Q: How many grams of cadmium metal will be deposited from a solution that contains Cd²+ ions if a…

A:

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

A:

Q: How much time is needed to deposit 1.0 g of chromium metal from an aqueous solution of CrCl3 using a…

A: Faraday's law of electrolysis draws a relationship between the amount of substance deposited by an…

Q: 3. A metallurgist wants to goldplate a thin sheet with the following dimensions: 1.5 in, x 8.5 in. x…

A: Q3) Given that : Dimensions of thin sheet = 1.5 in×8.5 in×0.0012 Thickness = 0.0020 in a) Initial…

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.