An electrolytic cell produces aluminum from Al2O3 at the rate of ten kilograms a day. Assuming a yield of 100%, how many moles of oxygen (O2) are being produced simultaneously?

Q: How many grams of magnesium are produced if a current of 4.50 A is passed through the electrolysis…

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Q: The reactions occurring at (i) anode, (ii) cathode, during working of a mercury cell. Why does the…

A: A voltaic cell is an example of electrochemical cell. It uses a chemical reaction to produce…

Q: 2. The electrolysis of aluminum oxide in molten cryolite to produce aluminum metal uses cells that…

A: Given: Current passed = 200000 A And mass of Al formed = 908 Kg = 908000 g…

Q: How much energy is consumed to produce 1.00 kg of magnesium by electrolysis of molten MgCl2 using a…

A: Given: Mass of magnesium = 1.00 kg Current                     = 1.5 x 103 A Voltage…

Q: An electrolysis cell that deposits copper (from Cu2+ ions) operates for 30 minutes at an electric…

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Q: Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If…

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Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 16…

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Q: Why does the electrolysis of an aqueous sodium chloride solu-tion produce hydrogen gas at the…

A: Electrolysis is a method of passing electric current through ionic or molten salt resulting in the…

Q: 3. A factory wants to produce 1.0 x 103 kg Barium from the electrolysis of molten barium chloride.…

A: The given values are: m=1.0×103 kg=1.0×106 gt=4.0 h=4.0 ×3600 s The electrolysis step to form barium…

Q: Which element is used to construct the standard half-cell?

A: Here given ,Multiple choice question

Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 15…

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Q: An electrolysis cell for aluminum production operates at 5.5 V and a current of 7.0 x 10° A.…

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Q: Aluminum is produced from the electrolysis of aluminum oxide dissolved in molten cryolite.…

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Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 17…

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Q: In the Hall-Heroult process, a large electric current is passed through a solution of aluminum oxide…

A: The equation of deionization for aluminum is

Q: Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If…

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Q: What would be formed by the electrolysis of an acidic iron(III) chloride solution? Show all possible…

A: The electrolysis of molten iron(III) chloride produces elemental iron and chlorine. Balanced…

Q: Electrolysis of water at room temperature yielded oxygen gas at platinum anode by using current of…

A: On electrolysis of water oxygen gas is evolved at anode. From 96500 C of electric charge moles of…

Q: Metallic magnesium can be made by the electrolysis of molten MgCl2.How many minutes are needed to…

A: According to Faraday’s first law, the chemical deposition which takes place during electrolysis is…

Q: Write a balanced equation to represent the electrolysis of molten sodium chloride. What volume of…

A: A balanced equation to represent the electrolysis of molten sodium chloride has to be given.

Q: Determine the mass of Sodium produced when a 22 amp current flows for 7 hr through a cell|…

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Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 15…

A: Using Faraday law of equivalent m = E.i.t. /F  Where E is equivalent mass of atom Z  = Atomic weight…

Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 12…

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Q: Aluminum metal can be made from aluminum(III) ions by electrolysis. What is the half-reaction at the…

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Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 17…

A:

Q: In the Hall-Heroult process, a large electric current is passed through a solution of aluminum oxide…

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Q: Calculate the mass of aluminum produced in 1.00 hour by the electrolysis of molten AlCl3 if the…

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Q: Electrolysis plays an important role in the manufacture or purification of all of the following…

A: There are different type of compounds, which are synthesized by different methods -  (1) Sodium, Na…

Q: In the Hall-Heroult process, a large electric current is passed through a solution of aluminum oxide…

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Q: In the Hall-Heroult process, a large electric current is passed through a solution of aluminum oxide…

A: Amount of pure aluminium formed can be calculated from the moles of charge passed.

Q: Predict the products of the electrolysis of an aqueous solution of sodium chloride in cell using…

A: Electrolysis is a spontaneous redox process Here we are required to find the product when aqueous…

Q: How many grams of chlorine can be produced by the electrolysis of mattersNaCl with a current of 1.02…

A: Given, Current 'i' = 1.02 A time 't' = 15 min

Q: an electrolytic cell produces aluminum from Ai2O3 at the rate of ten kilograms a day. assuming a…

A: Given: Mass of Al per day is 10 kg

Q: When does a SHE function as a cathode? As an anode?

A: Every electrochemical cell has a cathode and an anode. Each electrochemical cell has an oxidation…

Q: Aluminum is produced commercially by the electrolysis of Al203 in the presence of a molten salt. If…

A: Total current, I = 1.09 million Ampere                           = 1.09×106 Ampere Time, t = 3 hr…

Q: Which products are obtained in the electrolysis of molten NaI?

A: Na metal produced at cathode and I2 produced at anode.

Q: Enter your answer in the provided box. Copper is purified by electrolysis. A 4.75-kg anode is used…

A: Given:  Mass of anode = 4.75 kg = 4750 gm  Current (I) = 37.8 A

Q: Write the anode and cathode reactions occurring in a commonly used mercury cell. How is the overall…

A: The anode and cathode reactions occurring in a commonly used mercury cell and the overall reaction…

Q: In the Hall-Heroult process, a large electric current is passed through a solution of aluminum oxide…

A: we will apply the combined Faraday's law W = (Q*M )/F*n  W = weight of mass in grams Q = quantity of…

Q: What mass of copper could be electroplated on the cathode in an experiment were an average of 200 mA…

A: Charge passing through the cell is determined using the given formula.

Q: How many grams of silver are deposited at a platinum cathode in the electrolysis of AgNO 3 (aq) by…

A: Given: Current, I = 5.30A Time, t= 4.0hr = 4 x 60x 60 s = 14400s And we know, Equivalence mass of…

Q: mass

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Q: Calculate the mass of chlorine in grams that can be produced by the electrolysis of 50.0 kg of…

A: The electrolysis of sodium chloride takes place as follows: 2NaCl(aq) + 2H2O(l) → 2NaOH(aq)+ Cl2(g)+…

Q: What mass of silver would plate onto the cathode if a current of 7.9 A flowed through the cell for…

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Q: Aluminum metal is produced by electrolysis of Al½O; in molten cryolite (Na3AlF6). (a) If the…

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Q: t the cathode during the electrolysis of an aqueous solution of magnesium iodide, MgI2?

A: Electrolysis is the process of generation of chemical energy by the use of electrical energy for…

Q: According to the calculation, the electrolysis formed 0.107 mol M. During this time, 7.00 g M are…

A: Given: No. of mole of  (M ) = 0.107 mole Mass of ( M ) = 7 g   Find Molar mass of ( M )= ???

Q: A factory wants to produce 1.0 x 10³ kg Barium from the electrolysis of molten barium chloride. What…

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Q: Why are active metals such as Al obtained by electrolysis using molten salts rather than aqueous…

A: Electrolysis Electrolysis is a process that helps to bring chemical reactions into electrolytes.it…

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.