If a current of 5.00 A is applied for 96.00 minutes, how many grams of magnesium will be formed? Give me the answer in FOUR digits please :) MgCl2 → Mg + Cl2

Q: How many seconds are required to deposit 0.274 grams of manganese metal from a solution that…

A:

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: Faraday’s first law of electrolysis:                 The mass of the substance deposited at the…

Q: an acidic solution containing BiO+ is electrolyzed using a current of 0.500 A. what weight of Bi…

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

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

A:

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

A:

Q: 1. What is the maximum mass of copper that could be plated out by electrolyzing aqueous CuCl, for…

A: Using Faradays law of electrolysis we can solve this question.

Q: Determine the molar mass (amu) of Metal (M) if it took 2.05 minutes for a current of 1.91 A to plate…

A:

Q: Calculate Current or Time How many amperes are required to deposit 0.242 grams of silver metal in…

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Q: A zinc bar (atomic mass = 65.38 g/mol; ion charge = 2) is weighing 2.08 kg is attached to a buried…

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Q: A constant current of 9.25 amperes is passed through a cell containing iridium (III) nitrate,…

A: We have current as 9.250 A , time as 7.57 hrs, deposit of Ir is taking place, we have to calculate…

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

A:

Q: se a current of 770. mA flows through a copper wire for 10.0 minutes. Calculate how many moles of…

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

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Q: Enter your answer in the provided box. A constant current is passed through an electrolytic cell…

A: Faraday's first law :-  The mass of the substance deposited at electrode is directly proportional to…

Q: How many grams of zinc, Zn (s) are electroplated out of a solution containing Zn2+ (s the solution…

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Q: 1. A constant current of 90 mA is applied to an electrochemical cell for 22 minutes. What is the…

A: The charge transport in a unit time is known as electric current. The current is calculated by using…

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: 10

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Q: A factory wants to produce 1.00 × 10 kg barium from the electrolysis of molten barium chloride. What…

A: Electrolysis is a chemistry and industrial process that uses direct electric current (DC) to drive a…

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: The charge carried by one electron is 96500 C. The electrode reaction:

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: Determine the molar mass (amu) of Metal (M) if it took 2.85 minutes for a current of 1.1 A to plate…

A: Molar mass can be calculated as:-

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

A:

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: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

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

A:

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

A: Given: Time = 3.3 hours Current = 17.8 A Atomic mass of copper = 63.5 g/mol

Q: A gold (III) chloride solution was electrolyzed using a current of 13.5 amperes for four hours. How…

A: Mass deposit or plated  = Z.i.t

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

A:

Q: Suppose the current flowing from a battery is used to electroplate an object with silver. Calculate…

A: The electrochemical reaction of silver is –

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

A:

Q: How many grams of Ca metal (atomic mass = 40.08 g/mol) are produced by the electrolysis of CaBr2…

A: From the combination of Faraday's first and second law of electrolysis :  W/E = I*t/F  Or, W =…

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: The mass of aluminum metal calculated as follows

Q: How many seconds are required to deposit 0.221 grams of cadmium metal from a solution that contains…

A:

Q: Suppose that a machine part requires 400 mg of copper to provide a coating that is thick enough for…

A: Given data,Current=0.5ATime=10min=10×60s=600s

Q: Weighing a copper atom in an electrolysis experiment. A standard experiment involves passing a…

A: Electrolysis is the process through which electrical energy is converted into the chemical energy…

Q: How many hours would it take to reduce one mole of Al+3 to aluminum using a current of 22.2 Amps?…

A: Faraday's law of electrolysis states that the mass of metal produced or deposited at electrode is…

Q: decided to deposit 55.00 g of gold over an iron medallion by electroplating it from a solution…

A:

Q: How many seconds are required to deposit 0.252 grams of tin metal from a solution that contains Sn2*…

A: Mass of Sn = 0.252 g  Time = ?

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

A: In this question, we will determine the mass of Zn metal which is deposited from the Solution in…

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 5.1…

A: Solution: From the Faraday first law we have, the amount of chemical change being produced by a…

Q: A current was passed for 5 hours through two electrolytic cells connected in series. The first cell…

A: Chemical equations for the reduction of gold and copper ions are: Au3+(aq)+3e-→Au(s)…

Q: Consider an electrolytic cell with a steady current of 174 amperes which produces Als) (atomic mass…

A:

Q: How many minutes would be required to electroplate 20 g of chromium (52.00 g/mol) by passing a…

A: Let t be the time required in seconds than total charge passed in t seconds = current in ampere…

Q: How many minutes would a current of 20.0 amps need to run through a solution containing Au*3 to…

A: Amount of the current flow = 20A Mass of liberated substance = 10g Electron transfer per ion = 3

Q: Enter your answer in the provided box. A constant current is passed through an electrolytic cell…

A:

Q: How many minutes would it take to deposit all the  Al from 225 ml of 0.10 M   aluminum nitrate  with…

A: The given data contains, Molarity = 0.10 M. Volume = 225 ml. Current = 220 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.