How many seconds are required to produce 8.00g of aluminum metal from the electrolysis of molten AICI3 with an electrical current of 12.0A?

Q: (a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

A: Given, Current = 62.7 A Time = 81.9 min NaNO2 (aq) + H2O (l)     NO (g) + O2 (g) + NaOH (aq)…

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

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: A molten binary salt, Cal2, is electrolyzed. Write the half reactions that occur and identify which…

A: The binary salt given is CaI2  hence it has cation Ca2+ and anions I-

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to…

A: Equivalents of H+ ions reduced = QF=I×t96500=11.3 ×73 ×6096500= 0.513 Total equivalents of H+ ions…

Q: A certain half-reaction has a standard reduction potential Ed=+1.18 V. An engineer proposes using…

A: Standard reduction potential:

Q: A solution of a metal ion M 3+(aq) is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19…

A: The given data contains,       current =5 A      time =10 min60s1 min=600s

Q: A current of 11.8 A is applied to 1.25 L of a solution of 0.549 mol L- aqueous HBr converting some…

A:

Q: For the reaction : Als) / Al® aq) // Mg*?«aq) / Mg(s) the amount of cell potential produced is and…

A: The reaction :  Al(s) | Al3+(aq) || Mg2+(aq) | Mg(s)  Amount of cell potential produced = ?…

Q: All WOTK men A solution of NaCl (aq) is electrolyzed for 15.5 min using a current of 3.45 A. Write…

A: Given that, a solution of NaCl (aq) is electrolyzed. The time is t = 15.5 min = (15.5×60) sec = 930…

Q: Chrome is plated from solutions of chromium (III) chloride. If a current of 4.57 A is passed through…

A: Given that: Mass of chromium deposited = 14.5 g Amount of current passed through solution = 4.57 A…

Q: Copper is electroplated from CuSO4 solution. A constant current of 4.28 A is applied by an external…

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Q: During the discharge of an alkaline battery, 4.50 g of Zn is consumed at the anode of the battery.…

A:

Q: How many grams of Au would be deposited from an aqueous solution of Au 3+ with a current of 2.213 A…

A: Given, Molecular mass of Au = 196.96 u Current = 2.213 A time = 480 minutes = 28,800 sec

Q: Suppose a current of 690 mA is passed through an electroplating cell with an aqueous solution of…

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Q: What amount of Cu (in grams) is deposited at the cathode when a current of 6 A is maintained for 15…

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

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Q: If a water electrolysis cell operates at a current of 7.8 A, how longwill it take to generate 25.0 L…

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

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Q: A current of 3.86 A is passed through a Pb(NO,), solution for 1.60 h. How much lead is plated out of…

A: Faraday law of electrolysis states that the amount of substance deposited at the electrode is…

Q: 9. A concentrated Pb(NO3)2 (aq) solution is electrolyzed using a current of 10.5 A. a) What mass of…

A: SOLUTION: Step 1: Hello. Since the question contain multiple sub-parts, the first three subparts are…

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 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: 2+ A current of 3.40 A is passed through a solution containing Cu²+ (aq) for 30.0 minutes, with…

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Q: a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

A: Given data: Current = 67.8 A = 67.8 C/sec Time = 86.4 min = 86.4 x 60 sec Formula used: q = I x t

Q: 3. The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a Cuso,…

A: The Faraday's laws are the main concepts of electrochemistry.  The first law shows  the connection…

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: How many grams of Ag can be produced by passing a current of 0.350 A through a solution of AgNO3 for…

A: Faraday first law of electrolysis:  The mass of substance (m) deposited at an electrode is directly…

Q: What mass of copper could be deposited from a copper(II) sulfate solution using a current of0.50 A…

A: The given problem can be solved by using the formula as; Q=I×t…

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr, converting some of the H* to…

A: Given: Current (I) = 11.3 A     Volume of solution (L) = 1.25 L    Concentration of HBr = 0.552 M…

Q: Gold can be plated out of a solution containing Au3+ according to the following half-reaction: Au 3+…

A:

Q: Silver can be electroplated at the cathode of an electrolysis cell according to the following…

A: The charge and number of moles of silver is calculated as,

Q: What mass of Cu may be deposited from a Cu2+ solution during electrolysis by a current of 3.00 A for…

A: From the reaction it is clear that 1 mole Cu2+ requires 2 e-s fo the reduction of Cu2+ ions.…

Q: A current of 3.27 A is passed through a Pb(NO3)2 solution. How long, in hours, would this current…

A:

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

A: Electrolysis is a process in which current is passed through a substance .In this chemical reactions…

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 2.1…

A: We have given that during the electrolysis of molten Sodium chloride 2.1 g of Sodium is produced at…

Q: 1. A solution of a metal ion Mi) is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19 g…

A:

Q: In an electrolytic cell, how many grams of nickel (MM = 58.69 g/mol) will be deposited on a metal…

A: we have to calculate the mass of Ni deposited

Q: Silver can be electroplated at the cathode of an electrolytic cell by the half-reaction: Ag*(aq) + e…

A: According to Faraday's law ; The mass of the substance deposited on the electrode will be directly…

Q: a) A proposed battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a…

A: Hii there, since there are multiple questions posted. We are answering first question. If you need…

Q: How many minutes are required to deposit 1.34 g Cr from a Cr*(aq) solution using a current of 2.50…

A:

Q: A solution of a metal ion ÷({ ) Q˘ is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19…

A: Solution        1.a. Given that current,I=5.00A           time, t=10 minutes =10×60s…

Q: Chrome is plated from solutions of chromium (III) chloride. If a current of 4.57 A is passed through…

A: Given data:  Current = 4.57 A  Cr deposited = 14.5 g  Molar mass of Cr = 52 g.mol-  CrCl3  ==>…

Q: A current of 5.65 A is passed through a Cu(NO,), solution for 1.10 h. How much copper is plated out…

A: The balanced chemical reaction is as follows:

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 solution containing a metal ion (M+2, aq) is electrolyzed by a current of 7.8 A.  After 15.5…

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Q: A voltaic cell is constructed with two hydrogen electrodes. Electrode 1 has PH2 = 1.00 atm and an…

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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.

Q: If a current of 15 A is run through an electrolysis cell for 2.0 hours, how many moles of electrons…

A: First find number coulombs (C) charge  i.e  Q = i x t  Where  Q= charge in coulombs  i = current  in…

Q: During the electrolysis of a solution of Zn(NO3)2, 1.572 g of metal plated out at the cathode. How…

A: Given  Mass of Zn ( W )= 1.572 gram  Number of Coulombs ( Q )= ?

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.