current of 4.39 A is applied to a CuSO4 solution to deposit copper. Calculate the time it will take to deposit 1.00 x 107 g of copper

Q: A total of 1.740 F of electricity (1 F=1 mol e−) was required to electrodeposit all of the Zn and Co…

A: The mass of each compound is calculated by the number of moles of the compound. The number of moles…

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: An electrolytic cell contans 50.0 mL of a 0.152 M solution of FeCl3. A current of 0.775 A is passed…

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Q: How many grams of aluminum metal will be deposited from a solution that contains Alst ions if a…

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Q: How many seconds are required to deposit 0.239 grams of manganese metal from a solution that…

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Q: How much current is required to electroplate a metal surface with 0.432 g nickel metal from a…

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

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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: Manganese metal can be produced industrially by electrolysis of MnO2. How many hours would it take…

A: The compound of manganese electrolysed is MnO2 having Mn4+ ion. Hence the electrolysis reaction to…

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

A: Using Faraday's First of electrolysis: w = ZIt Z = Equivalent mass of metal96500w = Molar mass of Cu…

Q: A current of 4.71 A is passed through a Sn(NO3)2 solution. How long, in hours, would this current…

A: Given,Amount of current = 4.71 AMass of tin plate out = 5.10 gRequired,                   The time…

Q: Electrolysis of an NaCl solution with a current of 2.00 A for a period of 200 s produced 59.6 mL of…

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

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Q: How many grams of nickel metal will be deposited from a solution that contains Ni²+ ions if a…

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Q: Copper is plated onto the cathode of an electrolytic cell containing CuCl2(aq). How long does it…

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Q: An electrolytic cell produces aluminum from aluminum oxide, Al2O3. What mass of aluminum can be…

A: Applying formula w=Zit

Q: A constant current of 0.800A was used to electrolyze copper in an electrolytic cell, where copper…

A: Answer:- This question is answered by using the simple concept of electrolysis of a salt then mass…

Q: An aqueous solution of a platinum salt is electrolyzed for 1.00 hour using a current of 1.50 A to…

A: According to Faraday's law when a solution of an element is electrolysed then it will deposited.…

Q: 3.53 L of 0.362 M  solution are electrolyzed (Cu is plated out of solution as metal.) A current of…

A: NOTE: Assuming that the solution contains Cu2+ ions and the concentration data given is for the Cu2+…

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: How long will it take to plate 2.5 g of copper onto a light fixture using a solution of Cu(NO3)2 and…

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Q: Aluminum(III) ion (Al 3+) is reduced to solid aluminum at an electrode. If a current of 2.75 amperes…

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Q: If a constant current of 115 A is applied for 15.0 hours to the plating of cobalt from a cobalt(III)…

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

A: Mass can be calculated as:-

Q: The electrolysis of AℓCℓ3 at high temperature produces aluminium metal. If a constant electrical…

A: Given: current = 10 × 103 mA Or current = 10 × 103 × 10-3 A Or current = 10 A And time = 1 hour =…

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 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: How long, in minutes, will it take to produce 370.0 g of pure lithium by running a current of 330 A…

A: Given, Current passing = 330 A Mass of Li = 370.0 g  Molar mass of Li = 6.94 g/mol

Q: 05 g Ru is produced at the cathode, what is the charge on the ruthenium ions in solution?

A: Dear student I have given answer to your question in the image format.

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: An alternator recharges an automobile battery when the engine is running. If the alternator produces…

A: Given, Current produced by alternator = 1.540 A Engine operations requires = 1.179 A  mass of…

Q: How many hours are required to plate 12.00 g of nickel metal from 1.00 M NİSO4(aq), using a current…

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Q: How many grams of manganese metal will be deposited from a solution that contains Mn2+ ions if a…

A:

Q: How many grams of magnesium metal will be deposited from a solution that contains Mg2+ ions if a…

A: We have given that  How many grams of magnesium metal will be deposited from a solution that…

Q: How many grams of magnesium metal will be deposited from a solution that contains Mg2+ ions if a…

A: Weight of Mg deposited can be calculated using the equation of Faraday's first law. Answer is 0.2732…

Q: How many seconds are required to deposit 0.223 grams of lead metal from a solution that contains…

A: Given that, 0.223 grams of lead metal (Pb) is deposited from a solution that contains Pb2+ ions and…

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

A: Given:  Current = 0.974 A  Time = 67.4 min = 67.4 x 60 = 4044 sec

Q: What constant current would be needed for a copper cathode to accumulate 3.06 g of copper in 30 min.…

A: given- mass = 3.06 g. time = 30 min = 30 x60 = 1800 sec electrochemical equivalent of copper = 3.29…

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

A:

Q: How many seconds are required to deposit 0.184 grams of zinc metal from a solution that contains…

A:

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.