In the production of aluminum metal, Al^3+ is reduced to Al metal using currents of about 50,000 A and a low voltage of about 4.0V. Calculate how much energy (in kilo-watt-hours) is required to produce 2000, metric tons of aluminum metal.

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Q: An electrolysis cell for aluminum production operates at 5.0 V and a current of 8.5 x 10° A.…

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Q: What volumes of H2 (g) and O2 (g) at STP are produced from the electrolysis of water by a current of…

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Q: What mass of aluminum will be deposited in 1.00 hours by the electrolysis of molten AlCl 3 using a…

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Q: Molten RbCl can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

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Q: Molten RbCI can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

A: Given data: Weight of Rb = 23.4 g Current (A) = 1.25 A Equivalent weight of Rb = 85.461=85.46 Time…

Q: Purification of copper can be achieved by electrorefining copper from an impure copper anode onto a…

A: Current passed = 40 amp Mass of Copper to be deposited = 18.5 g Number of moles of Cu deposited =…

Q: Molten RbCl can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

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Q: How many hours does it take to form 15.0 L of O, measured at 750 torr and 30°C from water by passing…

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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: current =2.50 A Time = 1.90 hours  The calculation of the amount of charge is as follows: Charge =…

Q: In the commercial production of sodium metal by electrolysis, the cell operates at 7.0 V and a…

A: Given: Potential=7.0V current=25×103A Time=1h=3600s To find: The mass of metallic sodium produced in…

Q: Molten RbCl can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

A: we know the expression for the  faraday's law of electrolysis => m/E = It / F Where,  I is the…

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

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Q: Calculate the amounts of Cu and Br: produced at the inert elecuvues by passing a current of 4.5 A…

A: Given: Current = 4.5 A The atomic weight of Cu =63.55 gThe atomic weight of Br2=159.8 gCharge of 1…

Q: How many seconds does it takes to produce 5.0 L of aluminum sulfide, Al2S3 measured at 0.95 atm and…

A: Using ideal gas equation, we have P×V = n×R×T     -----(1) Where, P is pressure             , V is…

Q: Magnesium is obtained by electrolysis of molten MgCl2. Several cells are connected in parallel by…

A: In aqueous solution, H+, H2O, Mg2+, and Cl- ions are available and on electrolysis, hydrogen gas…

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: In the production of aluminum metal, Al³+ is reduced to Al metal using currents of about 50,000 A…

A: Given ,            I =50000 A            V =4 V             w =2000 metric tons i.e 2 ×109 g we know…

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: Molten RbCI can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

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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: Suppose 220. mmol of electrons must be transported from one side of an electrochemical cell to…

A: Given  mmol of electrons = 220  Time = 214 s  We have to calculate current

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

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Q: Which of the following substances will conduct electricity in both of its molten and solid states?…

A: As we know,  electricity is conducts due to free electrons and free ions   Sn is the element which…

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

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Q: How many grams of nickel metal can be plated from 1.00M NISO4(aq), using a current of 3.00 A for…

A: Here mass of metal is calculated by using faraday's law

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

A: Given:  Current (I) = 10 x 103 Amp  Time(t) = 1 hour = 3600 sec

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

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Q: A current of 5.90 A is passed through a Sn(NO3)2 solution. How long, in hours, would this current…

A: The solution is having salt Sn(NO3)2 which contains ion Sn2+  Hence on passing the current, below…

Q: A major source of sodium metal is the electrolysis of molten sodium chloride. What magnitude of…

A: The  current is required to produce 1.0 kg of sodium metal in one hour is calculated as,

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

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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: 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: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 2.35…

A: moles of electrons  =6.2x1018 x2.35x140x60/6.022x1023 =20454 x 10-5 =0.2 Moles of electron = number…

Q: Molten RbCl can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

A: Faradays first law of electrolysis :- The amount of the substance deposited at the electrodes is…

Q: A copper rod was purified using an electrolysis method consisting of a 1.0 M solution of copper (II)…

A: The correct answer is given below ?

Q: Aluminium metal can be made from aluminium ians by electrolysis. What mass of aluminium metal would…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: An electrolytic cell produces aluminum from Al2O3 at the rate of ten kilograms a day. Assuming a…

A: The formation of Al from Al2O3 is as follows: 2Al2O3(s)→4Al(s)+3O2(g) Calculation of no. of mol of…

Q: What mass of aluminum can be plated onto an object in 378 minutes at 5.80 A of current?…

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

Q: In the production of aluminum metal, Al³+ is reduced to Al metal using currents of about 50,000 A…

A:

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.

Q: You pass a 2.5 amp current through an aqueous solution of aluminum nitrate for 5 hours. How many…

A: Aluminium nitrate Al(NO3)3 has Al3+ ions Al3+ + 3 e-  -----> Al So to reduce 1 mole Al3+ ions to…

Q: An electrolysis cell for aluminum production operates at 4.5 V and a current of 7.5 x 10° A.…

A:

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

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Q: Why is it not possible to plate a metal spoon with aluminium using 1.0M Al(NO3)3 (aq)?

A: In aqueous solution, water and aluminum salt is present. When a metal spoon will be kept here that…

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A: When 96500 coulombs are passed through a solution of NaCl, one mole of chlorine is deposited.

Q: Magnesium metal can be produced via the electrolysis of molten magnesium chloride harvested from…

A: a.) The molten MgCl2 contain two type of ions Mg2+ and Cl-. The magnesium ions undergo reduction to…

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 2.30…

A: In the electrolysis process, the grams of Chlorine gas generated is calculated using,

Q: How many hours does it take to form 15.0 L of O2 measured at 750 torr and 30°C from water by passing…

A: According to Faraday's first law ,when current is passed through an electrolytic solution, the…

Q: An electrolysis cell for Aluminum production operates at 4.5V and a current of 1.5 x 10 A. Calculate…

A: Given the current passed, I = 1.5*105 A Potential, V = 4.5 V  Mass of Al(s) needs to be produced =…

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.