A constant current of 0.712 A is passed through an electrolytic cell containing molten BaCl2 for 10.6 h. What mass of Ba(s) is produced? The molar mass of barium is 137.3 g/mol. Provide your answer rounded to 3 significant digits.

Q: How long will it take to plate out 3.9 g Ni from aqueous Ni2+ with a current of 108.2 A? HOW DO WE…

A: To plate Ni using the process of electrolysis, the reaction that needs to be employed on the…

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: How long will it take for a uniform current of 6.00 A to deposit 78.0 g gold (197.0 g/mol) from a…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu²* (aq)+…

A: The reaction given is, Cu2+aq+Zns→Cus+Zn2+aq Cu2+ is being reduced to Cu and Zn is being oxidised to…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: Current =5.00×10^2A Mass of chlorine=4.18kg=(4.18×1000)g=4180g

Q: How long would it take to electroplate all the Zn^ 2+ in 0.280 L of .210 M ZnSO 4 solution with a…

A: The question is based on the concept of electrochemistry. It involves  application of first law of…

Q: How long in seconds would it take to deposit 59.07 g of Pt from an aqueous solution of Pt 2+ with a…

A:

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: How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous…

A: The balanced chemical equation for the reduction of copper is: Thus, for the production of 1 mole…

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 long (in hours) must a current of 4.61 amps be passed to produce 79.5 g of copper metal from a…

A: Given:: Current i= 4.61 A  Mass of Cu = 79.5 g  Molar mass of Cu= 63.55 g mol-1 Time t= ?

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

A:

Q: Manganese metal can be produced industrially by electrolysis of MnO2. How many hours would it take…

A: The compound of manganese electrolysed is MnO2 having Mn4+ ion. Hence the electrolysis reaction to…

Q: Determine the current (in A) to produce 3.10 g Ag when Ag"(aq) is electrolyzed for 2.00 h. (F =…

A:

Q: How long, in hours, must a current of 5.00 A be applied to a solution of Ag+ to produce 10.5 grams…

A: From the combination of Faraday's first and second law, we have : m = ItM/Fz  Or, t = mFz/IM ...(1)…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn"…

A: The reaction given is Hence in the above reaction, Sn2+ is being reduced to Sn and Ba is being…

Q: How long would it take to deposit 3.75 g of iron from an aqueous solution of iron (III) sulfate by…

A: According to Faraday's First Law of Electrolysis, the chemical deposition due to flow of current…

Q: How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with a current of 105.9 A? HOW DO WE…

A: Given: Mass of Ni to be plated out = 1.0 g. Current pass = 105.9 A.

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

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

Q: A solution containing a 3+ metal ion is electrolyzed by a current of 5.0 A for 10 minutes. What is…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Sn*(aq)…

A: Given cell reaction  Sn2+(aq) + Ba(s) ----> Sn(s) + Ba2+(aq) At Ba electrode oxidation taking…

Q: Calculate the mass in grams of a metal Q ( Molar mass= 88.23 g/mol) that will be deposited from a…

A:

Q: 1. What is a cell potential? 2. In what way does a galvanic cell becomes an electrolytic cell?

A: Galvanic cell is the spoteneous redox reaction where chemical energy transferred to electrical…

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

A:

Q: Determine the molar mass (amu) of Metal (M) if it took 2.95 minutes for a current of 1.8 A to plate…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Sn…

A: The cell reaction taking place is given as, => Sn2+ (aq) + Ba (s) -------> Sn (s) + Ba2+ (aq)…

Q: Tin-plated steel is used for "tin" cans. Suppose that in the production of sheets of tin-plated…

A:

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: How long, in minutes, will it take to produce 370.0 g of pure lithium by running a current of 330 A…

A: Given, Current passing = 330 A Mass of Li = 370.0 g  Molar mass of Li = 6.94 g/mol

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 alternator recharges an automobile battery when the engine is running. If the alternator produces…

A: Given, Current produced by alternator = 1.540 A Engine operations requires = 1.179 A  mass of…

Q: ulate the potential of the following cells: a galvanic cell consisting of a lead electrode on the…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Sn n²* (aq)…

A:

Q: What mass of each of the following substances can be produced in 1.4 h with a current of 10. A? (a)…

A:

Q: How long must a current of 5.00 A be applied to a solution of Ag + to produce 10.5 g silver metal?

A: The electrolysis reaction taking place to produce Ag (s) from Ag+ (aq) solution will be  Ag+ (aq) +…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn²+…

A:

Q: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

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: 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: A pure organic acid sample (0.1516 g) is neutralized with OH- ions produced in a constant current of…

A:

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

A: Interpretation -  In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are…

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

A:

Q: Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive)…

A: Electroplating is a process of coating layer of metal over another metal by the process of…

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

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn…

A:

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

A:

Q: How many seconds are required to deposit 0.150 grams of tin metal from a solution that contains Sn2+…

A: Mass = 0.150 g Current (i) = 0.652 A = 0.652 C/s  Time (t) = ?

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.