How long will it take to plate out each of the following with a current of 100.0 A?  1.0 kG Al from aqueous Al3+   (book answer: 30 hours) 1.0 g Ni from aqueous Ni2+     (book answer: 33 s)

Q: Calculate the E cl for the following reactions and state if the given cell is either a galvanic or…

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Q: A current of 3.79 A is passed through a Sn(NO^), solution. How long, in hours, would this current…

A: Oxidation is the process that involved the loss of electrons and oxidized to cation.  Hence when a…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: When both the standard Reduction potential are given , then we have to see the more positive…

Q: Write a balanced overall reaction from these unbalanced half-reactions. Cu → Cu²+ Ag+ → Ag -

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Q: For the cell at 320 K outlined below, answer the questions. Each cell has a volume of 100.0 ml…

A: Given Cell Au (s) | Au3+ (0.05 M) || Au3+ (1.2 M)|Au Temperature- 320 K Volume- 100.0 ml Current-…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Cu²+ (aq)…

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Q: The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76…

A: Zn (s) +  2H+ (aq) → Zn2+ (aq) + H2 (g)Standard cell potential (Eo) = 0.76 VCCell potential (E) =…

Q: Ate Shawol and Concertina performed electrolysis to determine the identity of an unknown metal X.…

A: One mole of electrons has a charge of 96500 C. This quantity of electricity is called one faraday.…

Q: cator=assighment-lake [Review Topics] [References] CHEMWORK An electrolytic cell is set up to plate…

A: Introduction: As we know that the Michael Faraday described the quantitative aspects of Electrolysis…

Q: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.46 A of current for 1.00 h.…

A: Oxidation takes place at anode.  So, metal will be eroded from anode.  Thus, minimum mass of anode…

Q: A certain half-reaction has a standard reduction potential Ered=-0.70 V. An engineer proposes using…

A: The cell potential needed by the engineer is 1.40 V or greater. The reduction potential of…

Q: help please answer in text form with proper workings and explanation for each and every part and…

A: Step 1: Identify the Oxidation and Reduction Half-ReactionsIn a redox reaction:Oxidation occurs at…

Q: An electrolytic cell is set up to plate Zr(s) from a solution containing Zr4+(aq). A current of 7.59…

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Q: How many milligrams of primary cathodic material is produced if aqueous FeCl3 solution is…

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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: What half-cell reaction is shown by the equation C12 + 2e- --> 2CI -? * O chemical reaction O redox…

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Q: 29

A: We have given that  How much time (in hours) is required to produce 2.20 kg of Zn(s) from a solution…

Q: A current of 0.950A passed for 21.0min through a CuSO4 solution. Calculate the amount of copper…

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Q: otentials. 2 +2H2O + 4e --> 40H Enote = 0.401V a2+ 2e ----> Ca Enote = -2.868 alculate the maximum…

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Q: Propose a metal cathode for an electrochemical battery with an anode Tin (2+) using the standard…

A: Since at cathode reduction takes place and at anode oxidation. Hence the reaction taking place at…

Q: What current must be used to plate 1.75 moles of copper on an electrode in 6.25 minutes?

A: ∙Given:-  no. of moles of copper =1.75 moles                     Time =6.25  minutes or  375s

Q: help please answer in text form with proper workings and explanation for each and every part and…

A: Step 1: Step 2: Step 3: Step 4:

Q: From the standard electrode potentials table of the cell: Ca I Ca2+ || Zn2+ I Zn calculate AG°…

A: Ered°, Ca2+/Ca=-2.866 VEred°, Zn2+/Zn=-0.76 VAt anode,Ca→Ca2++2e-At cathode,Zn2++2e-→Zn…

Q: A voltaic cell using Pb2+/Pb and Ni²+/Ni half-cells is set up at standard conditions, and each…

A: Answer:Voltaic cell is a type of electrical cell that converts chemical energy into electrical…

Q: How much time in minutes would it take to deposit 1.05 grams of X (MW = 64.75 g/mol) on a cathode in…

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Q: A 1.00 g of metal sample took 31.05 minutes to be consumed in the anode to recharge a battery using…

A: According to Faraday's first law of electrolysis, the mass of a substance deposited on the electrode…

Q: How long (in minutes) should a current of 5.6 amperes be applied through a solution of silver…

A: According to Faraday's first law mass of substance deposited on electrode is proportional to the…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: Oxidation reaction takes place at anode and reduction takes place at the cathode. Oxidation can be…

Q: 2. Ate Shawol and Concertina performed electrolysis to determine the identity of an unknown metal X.…

A: Given: current=1.495 Atime=18.00 hrsmass of metal=17.81 gnumber of electrons=3 e- To find: Unknown…

Q: cell has a standard cell potential of 0.177V at 298K. What is the value of the equilibrium constant…

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Q: The redox reaction below has a AG value of 642. kJ. Determine the standard cell potential (E cell)…

A: Given that, a balance redox reaction is A(s) + 5B3+(aq) → A5+(aq) + 5B2+(aq). The ∆G0 value of the…

Q: The electrolysis of molten AICI3 for 2.50 hr with an electrical current of 12.0 A produces g of…

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Q: How long (in minutes) should a current of 6 amperes be applied through a solution of silver nitrate…

A: It is an application of Faraday  first law of electrolysis

Q: Suppose the galvanic cell sketched below is powered by the following reaction: Zn(s)+NiCl₂(aq) 4…

A: Given information:

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: Given: The reactions in two two half cells are as follows: Fe3+aq+e-→Fe2+aq   E°=+0.771 V......(1)…

Q: Check Your Understanding Suppose that a machine part requires 400 mg of copper to pro- vide a…

A: Solution:     Electroplating is a method of coating one metal onto the other with the help of an…

Q: What volumes of H2₂(9) and O₂(g) at STP are produced from the electrolysis of water by a current of…

A: Given process: electrolysis of watercurrent = I = 2.64 ATime = t = 15.5 minCondition : STPVolume of…

Q: Consider a galvanic cell for which the anode reaction is Pb(s) → Pb+2 (0.010 M) + 2e- , E= -0.1263…

A: According to guidelines we are supposed to answer only first three subparts. If you want rest of the…

Q: 4.) How long would it take (in min) to plate 29.6 g of nickel from a 1.0 M Ni2* solution using a 4.7…

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Q: help me asap and pls pls make sure your answers are all correct, thanks

A: In Galvanic cell,  Oxidation takes place at anode and reduction takes place at cathode.  E°cell =…

Q: Is there a minimum standard reduction potential that the half- reaction used at the cathode of this…

A: Approach to solving the question: there is a minimum standard reduction potential, but there is no…

Q: Use the data in Appendix D in the textbook to calculate the standard cell potential for each of the…

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Q: How much time is needed for a 1.00 g Ag to be deposited by electrolysis of a AgNO3 solution using a…

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Q: Pls help ASAP.

A: Select the incorrect statement :

Q: How many hours are required to produce 795 grams of lead from molten lead(II) chloride (PbCl2, 278.1…

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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.