QUESTION 15 If a constant current of 1.50 x 108 A is passed through a molten mixture of aluminum oxide and cryolite for 4.00 hour kg of aluminum can be produced. Enter your answer as the nearest whole number, (value t 296).

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 3.12 A3.12 A is passed through a Sn(NO3)2Sn(NO3)2 solution for 1.20 h1.20 h. How much…

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Q: How many minutes will it take for a current of 10.4 A to deposit 4.06 g of gold from a solution of…

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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: What mass of silver would plate onto the cathode if a current of 6.7 AA flowed through the cell for…

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Q: Determine the molar mass (amu) of Metal (M) if it took 2.21 minutes for a current of 1.24 A to plate…

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

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Q: A current of 5.26 A is passed through a Pb(NO3)2 solution for 1.20 h. How much lead (in g) is plated…

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Q: How many seconds are required to deposit 0.224 grams of manganese metal from a solution that…

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Q: Three electrolytic cells are connected in a series. The electrolytesin the cells are aqueous…

A: The given data contains, current = 2.33 A. Mass of Cu = 1.74 g.

Q: How many milligrams of primary cathodic material is produced if aqueous FeCl3 solution is…

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Q: How many grams of mercury metal will be deposited from a solution that contains Hg2+ ions if a…

A: Given :  Current (I) = 0.599 A  Time(t) = 28.4 min = 28.4 x 60 sec = 1704 sec  Molar mass of Hg =…

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

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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: Determine the current (in A) to produce 3.10 g Ag when Ag"(aq) is electrolyzed for 2.00 h. (F =…

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Q: [Review Topics] [References] An electrochemical cell consists of a standard hydrogen electrode and a…

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Q: A current of 4.15 A is passed through a Pb(NO3)2 solution for 1.50 h. How much lead is plated out of…

A: Given that:  Current(I) = 4.15A = 4.15C/s  Time(t) = 1.50h = 1.50h×3600s/h = 5400s Reaction:  Pb2+ +…

Q: A current of 5.83 A is passed through a Fe(NO3)2 solution for 1.60 h. How much iron is plated out of…

A: According to Faraday's law of electrolysis, the amount of substance deposited on an electrode is…

Q: Determine whether the alkene shown below has a cis or a trans orientation around the double bond. O…

A: We have given the organic compound alkene and we have to determine whether the alkene has cis or a…

Q: How much time in minutes would it take to deposit 1.05 grams of X (MW = 64.75 g/mol) on a cathode in…

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Q: A Cr3+1aq2 solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out…

A: Charge flowing per unit time is known as current which may be expressed mathematically as :…

Q: Determine the current (in A) to produce 4.50 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

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Q: What current must be supplied to deposit 4.77 g of gold from a solution of AuCl 3 in 27.2 min?

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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: A current of 4.30 A is passed through a Pb(NO3)2 solution for 1.80 h. How much lead is plated out of…

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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: What mass of Iron, Fe, will be produced in a cell using Fe(NO3)3 if a current of 5.0A is maintained…

A: Given, Current flow = 5 A, Time = 2 hours = (2 * 3600)…

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

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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: 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 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: How many grams of Ag would be deposited from an aqueous solution of Ag+ with a current of 2.534 A…

A: Molar mass of Ag = 108g/mol Reaction takes place:- Ag+ + e-  ------> Ag  current , I = 2.534 A…

Q: A current of 3.33 A is passed through a Sn(NO3)₂ solution for 1.30 h. How much tin is plated out of…

A: We have to calculate mass of tin deposited on the plate

Q: A current of 4.63 A4.63 A is passed through a Pb(NO3)2Pb(NO3)2 solution for 1.30 h1.30 h. How much…

A: Amount of substance deposited at electrode during electrolysis can be calculated as follows

Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

A: According to electro-chemistry  W = zCt W= mass of Metal deposited in grams C= current  t = time in…

Q: Be sure to answer all parts. Draw the products formed when 2-propanol [(CH3)2CHOH], the main…

A: Conjugate acid has one more H and one more positive charge than the base that formed it.A conjugate…

Q: How many seconds are required to deposit 0.177 grams of manganese metal from a solution that…

A: Approach to solving the question: Detailed explanation: Examples: Key references:

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

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Q: If a current of 5.00 A is applied for 96.00 minutes, how many grams of magnesium will be formed?…

A: To find weight of magnesium

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: Use the data in Appendix D in the textbook to calculate the standard cell potential for each of the…

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Q: current of 2.505 A deposits 1.371 g of a metal M from a solution that contains the metal ion M²⁺ in…

A: Given, current (i) = 2.505 A Time (t) = 30 × 60 = 1800 s Mass = 1.371 g  Using Faraday's law,  Mass…

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

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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: What period of time (in hours) is required to produce 1.00mol of chlorine using a current of 5.00A?

A: A numerical problem based on Faraday's law, which is to be accomplished.

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.