In the Hall-Heroult process, a large electric current is passed through a solution of aluminum oxide  Al2O3  dissolved in molten cryolite  Na3AlF6 , resulting in the reduction of the  Al2O3  to pure aluminum.   Suppose a current of  920.A  is passed through a Hall-Heroult cell for  86.0  seconds. Calculate the mass of pure aluminum produced.   Be sure your answer has a unit symbol and the correct number of significant digits.

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

A:

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

A:

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…

A:

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…

A:

Q: The electrolysis of TℓBr3 at high temperature produces thallium metal. If a constant electrical…

A: From Faradays first law, weight of the substance deposited, W = ZQ Z = E/F = equivalent…

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

A: Answer :- 337.7 h The time take to plate 14.0 kg of Cu onto the cathode when 35.0 A current passed…

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: Copper metal can be purified electrolytically according to the following arrangement. The anode is…

A: W = I × t × M / n × F Where ; W = mass of  purified Cu = ? I = current = 15 A  t = time = 8.5 hours…

Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 20…

A: 3.4 amperes is 3.4 coulombs per second, 5C/s So the total charge in 20 minutes is Q = 3.4C/s x 20min…

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

A: Here given ,Multiple choice question

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

A:

Q: Calculate the number of grams of aluminum produced in 1.00 h by the electrolysis of molten AlCl3 if…

A: Given: Electrical current = 10.0 A Time of electrolysis = 1.00 h.

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

A:

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

A:

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: 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: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 14…

A: Given,

Q: Elemental calcium is produced by the electrolysis of molten CaCl2. (a) What mass of calcium can be…

A: Given: Current applied  = 7.5 x 103 A Time of supply   = 48 h Efficiency of cell = 68%

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

A:

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

A:

Q: Calculate the quantity indicated for each of the following electrolysis. a. The mass of Zn deposited…

A: The mass of zinc can be calculated by using Faraday's law of electrolysis.

Q: Electrolysis of a solution of Zn(NO3)2(aq) to give zinc metal is carried out using a currentof 2.12…

A:

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

A:

Q: Enter your answer in the provided box. The MnO, used in alkaline batteries can be produced by an…

A: Please find the answer attached here as handwritten note.

Q: An electrolysis cell for aluminum production operates at 4.0 V and a current of 8.5 x 10° A.…

A: The solution is given below -

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…

A:

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

A:

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…

A:

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

A:

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: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A: To produce gallium, gallium oxide which has Ga(III) ion is being reduced. Hence the electrolysis…

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: The electrolysis of molten potassium bromide, KBr, generates bromine gas which can be used in…

A: The production of Br2 from KBr- KBr aq →K+ aq+ Br-aq2K+aq + 2Br-aq→2Ks + Br2g

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: Calcium metal is obtained by direct electrolysis of molten CaCl2. If a metallurgical electrolysis…

A: Calcium metal is obtained by direct electrolysis of molten CaCl2. If a metallurgical electrolysis…

Q: If 25 amperes of current flow for 15 minutes through a solution of Sn(NO3)2, how many grams of tin…

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

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

A:

Q: In the electrolysis of molten MgCl 2, what mass of Mg metal is deposited by a current of 16 amperes…

A: Electrolysis is the process of conversion of electrical energy to chemical energy. This reaction…

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

A:

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: When zinc is refined by electrolysis, the desired half-reaction at the cathode is Zn²⁺(aq)…

A: Metals are found in the earth crust having lots of impurities with them in form of compound while…

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

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

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

A: Given; The reaction is as follows; Al3+aq+3e-→Als Charge on one mole of electrons=1Faraday 1 Faraday…

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.