Tin-plated steel is used for "tin" cans. Suppose that in the production of sheets of tin-plated steel, a line at a factory operates at a current of 100.0 A for exactly 8 hours on a continuously fed sheet of unplated steel. If the electrolyte contains tin(II) ions, what is the total mass of tin that has plated out in this operation?

Q: How many moles of oxygen, O2, will be produced by the electrolysis of water with a current of 1.5…

A:

Q: Magnesium metal can be produced industrially by electrolysis of MgCl2. What mass of magnesium metal,…

A:

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: A metallic object to be plated with copper is placed in a solution of CuSO.. What mass of copper…

A: Given,  Current, I = 0.22 amp  Time, t = 1.5 hours               = 5400 sec  Molar mass of Cu =…

Q: If the given statement is true, write T. Otherwise, write F and explain why it is false. 1) The…

A: Given the statement: The electrons in a galvanic cell can be transferred through a wire, making it…

Q: How many grams of gold will be plated out by a current of 0.35 A applied for 65 minutes from a…

A:

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 can be produced per hour in the electrolysis of a molten aluminum salt by…

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

A:

Q: How many moles of oxygen, O 2, will be produced by the electrolysis of water with a current of 1.5…

A:

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: The mass of three different metal electrodes, each from a different galvanic cell, were determined…

A: The active electrode which is found to lose mass during redox reaction in a cell is termed as anode…

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: state and explain Faraday’s laws of electrolysis. What is Electrochemicalequivalent?

A: Faraday’s first law of electrolysis states that the mass of the substance accumulated or released at…

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: If a salt bridge contains KNO3 as its electrolyte, which ions diffuse into solution in the anode…

A: A galvanic cell is an electrochemical cell that is used to supply electric current through the redox…

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

A: The faraday's first law explains that the quantity of any species deposited is directly proportional…

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: the electromotive force of a galvanic cell constructed of a standard hydrogen electrode and a lead…

A: The electrode potential when the concentration of all the half cells involved is unity is called the…

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: An aqueous solution of a platinum salt is electrolyzed for 1.00 hour using a current of 1.50 A to…

A: According to Faraday's law when a solution of an element is electrolysed then it will deposited.…

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

A: Since in the above reaction we can see that 1 mole of Cl2 is produced with 2 moles of electrons…

Q: A student was asked to set-up a galvanic cell in the laboratory. He used two copper electrodes, one…

A:

Q: (a) Liquid H2O is subjected to electrolysis. One of the half-reactions is 2 H2O → O2 (g) + 4 H+(aq)…

A: We have to calculate the Faraday of electricity required and the time taken.

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 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: 1.Chrome is plated from solutions of chromium (III) ions. If a particular application requires 13.7…

A: Since you have asked multiple questions in a single upload, if you want the second question to be…

Q: A constant current of 90 mA is passed for 22 minutes into an electrolysis cell. How much electrical…

A: Charge passing per unit time is known as  electric current.

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: In a galvanic cell, a full redox reaction takes place, one half-reaction at each electrode. How is…

A:

Q: How many hours are required to plate 12.00 g of nickel metal from 1.00 M NİSO4(aq), using a current…

A:

Q: standard potential

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 gold (III) chloride solution was electrolyzed using a current of 13.5 amperes for four hours. How…

A: Mass deposit or plated  = Z.i.t

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: How many seconds are required to deposit 0.184 grams of zinc metal from a solution that contains…

A:

Q: Over a period of time, the concentration of sulfuric acid in the lead storage battery of an…

A: Given data,Initial % by mass of H2SO4=38.0 %Final % by mass of H2SO4=26.0%Volume of H2SO4=734…

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) 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: A 0.1 M aqueous CaCl, solution is electrolyzed by usina inert electrodes. If 1.25 ampere current is…

A: At cathode this reaction is taking place,Ca2+  +  2e-   →  Ca  Calculate the charge first,Q = it and…

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: Weighing a copper atom in an electrolysis experiment. A standard experiment involves passing a…

A: Electrolysis is the process through which electrical energy is converted into the chemical energy…

Q: How much Beryllium metal can be deposited from a solution of BeCl2 by a current of 5.0 Amperes that…

A:

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

A:

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A: Given-> Current (I) = 1.48 ampere  Time (t) = 37.4 min = 37.5 × 60 second = 2250 seconds Weight…

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.