How many minutes would a 5.0 amperes current have to be applied to plate out 8.00 grams of copper metal from aqueous copper(ll) sulfate solution? Atomic wt. of Cu = 63.55 g/mol A 14.6min B 124 min 33.3 min D 81.0 min

Q: An aqueous solution of nickel acetate is electrolyzed for 3 hours with a 1.3 ampere current. What…

A: We know that  Mass = Z.I.t

Q: A current of 3.05 A is passed through a Pb(NO3)2 solution. How long, in hours, would this current…

A:

Q: A current of 3.66 A is passed through a Cu(NO3)2 solution. How long, in hours, would this current…

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Q: A steady current of 4A is maintained for 10.0 min. in a solution of silver nitrate. Find how much…

A: Given: Current = 4 A Time = 10.0 min Electrochemical equivalent of silver is 1.1180 x 10– 6 kg/C

Q: If a constant current of 2.0 amperes is passed through a cell containing Cr3+ for 1.0 hour, how many…

A: Mass of Cr deposited can be calculated using Faraday's first law of electrolysis: Mass deposited=…

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

A:

Q: An unknown metal M is electrolyzed. It took 672.8 s for a current of 2.50 A to plate out 0.121 g of…

A:

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

A:

Q: Suppose you are given a 1M solution of SnCl2 and another 1M solution of MgCl2. Leaving the…

A: The question is based on concept of redox chemistry. we have to determine the concentration of tin…

Q: What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr₂(SO4)3 for 185…

A: mass of chromium (Cr) deposited = ?Current = 10.0 ATime = 185 min = 185 × 60 s = 11100 s1 F = 96485…

Q: A tub of water containing Cr³⁺(aq) is subjected to a current of 1.0 amperes for 60 minutes. How many…

A: An external source of voltage is used to carry out a reaction in case of electrochemical cell. The…

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: A current of 3.66 A is passed through a Cu(NO3)2 solution. How long, in hours, would this current…

A: Faraday Law of Electrolysis  To find time for the certain amount of Copper deposition  solution…

Q: If 2.19 g of chromium metal was deposited from a solution of Cr3+ using a current of 35.2 amps in an…

A: Given, If 2.19 g of chromium metal was deposited from a solution of Cr3+ using a current of 35.2…

Q: Chromium is electroplated from CrPO4 solution. A constant current of 13.5A is applied by an external…

A: According to the first law of Faraday, the mass of metal deposited at the anode is given by: m = E I…

Q: An unknown metal M is electrolyzed. It took 672.8 s for a current of 2.50 A to plate out 0.121 g of…

A: According to Faraday’s first law, the mass of the substance (m) deposited or liberated at any…

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

A:

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

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

A:

Q: 32. What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for…

A: Given that,time, t = 244.7 min = 244.7 x 60 sec = 14682 seccurrent, i = 13.6 A F = 96485…

Q: What mass of copper could be deposited from a copper(II) sulfate solution using a current of0.50 A…

A: The given problem can be solved by using the formula as; Q=I×t…

Q: How many grams of zine metal will be deposited from a solution that contains 2+ Zn ions if a current…

A: The charge is directly proportional to the current and time associated with it. According to…

Q: What volumes of H3(g) and O,(g) at STP are produced from the electrolysis of water by a current of…

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

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Q: Ate Shawl and Concertina performed electrolysis to determine the identity of an unknown metal X.…

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Q: The electrolysis of 0.500 L of molten ZnCl2 will take place. Determine the current (amperes) needed…

A: According to Faraday's law of electrolysis -The amount of substance deposited at the electrode is…

Q: How many grams of copper will be plated out by a current of 2.3 A applied for 35 minutes to a…

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Q: A current of 4.05 A is passed through a Cu(NO3)2 solution for 1.70 h. How much copper is plated out…

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Q: What volumes of H2₂(9) and O₂(g) at STP are produced from the electrolysis of water by a current of…

A: Given process: electrolysis of watercurrent = I = 2.64 ATime = t = 15.5 minCondition : STPVolume of…

Q: A solution containg 75.0 mg copper was electrolyzed at a constant current of 0.250 A, causing…

A: Faraday's first law :  The amount of substance deposited is directly proportional to quantity of…

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

A: The given data is as follows: The current applied (I) = 1.10 A The time (t) = 32.1 minutes = 32.1×60…

Q: An aqueous solution of nickel acetate is electrolyzed for 3 hours with a 1.8 ampere current. What…

A: Given,  An aqueous solution of nickel acetate is electrolyzed for 3 hours with a 1.8 ampere current.…

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: How many grams of silver will be obtained when the aqueous silver nitrate solution is electrolyzed…

A:

Q: If a constant current of 2.0 amperes is passed through a cell containing Cr³+ for 1.0 hour, how many…

A: Given-> Current (I) = 2.0 ampere Time (t) = 1.0 hour = 1.0 × 60× 60 second = 3600 s Atomic mass…

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

A:

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 an electrolytic cell, how many grams of nickel (MM = 58.69 g/mol) will be deposited on a metal…

A: we have to calculate the mass of Ni deposited

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.