A current of 3.58 A is passed through a Ni(NO,), solution. How long, in hours, would this current have to be applied to plate out 6.40 g of nickel?

Q: Complete the following on paper, SHOWING ALL WORK. Al3+ is reduced to Al(s) at an electrode. If a…

A: As per the question balance chemical equation is as follows:         Current (I)= 2.00 ampere…

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: How many grams of silver metal will be deposited from a solution that contains Ag+ ions if a current…

A: As per the given information the balanced chemical cathode half reaction is as follows:…

Q: 7. How long has a current of 5 amperes to be applied through a solution of copper nitrate  to coat a…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Which of the following has the greatest tendency to be oxidized? (You may consult a table of…

A: Redox reaction :  The chemical reaction in which reduction and oxidation takesplace simultaneously…

Q: A 5.77 g of zinc is deposited at the cathode when a current of 7.1 amperes passes through an…

A: Given : Current = 7.1 A And time = 40 min = 40 X 60 = 2400 s…

Q: How long would it take to electrodeposit all the Cu2+ in 0.300 L of 0.230 M CuSO4 solution with an…

A: Given, 0.300 L of 0.230 M CuSO4 solution Applied potential difference of 0.275 V  Current of 3.50…

Q: How many grams of nickel metal will be deposited from a solution that contains Ni?+ ions if a…

A:

Q: (b) A constant current was passed through a solution of AuCl; between gold (Au) electrodes. After a…

A: Given, Mass of gold deposited = 2.628g Time = 20min = 1200 second

Q: How much current is required to electroplate a metal surface with 0.432 g nickel metal from 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: A current of 5.31 A is passed through a Fe(NO,), solution. How long, in hours, would this current…

A:

Q: How many seconds are required to deposit 0.266 grams of cadmium metal from a solution that contains…

A:

Q: A current of 4.90 A is passed through a Cu(NO,), solution. How long, in hours, would this current…

A: The chemical deposition due to the flow of current through an electrolyte is directly proportional…

Q: What is galvanization? How doesgalvanizing iron protect it from corrosion?

A: Corrosion is a natural process that deteriorate the quality of metal by forming an oxide layer over…

Q: A current of 3.62 A is passed through a Sn(NO,), solution. How long, in hours, would this current…

A: Formula used :-    W = E×c×t\F  Where E = equivalent mass of the ion              c = Current passed…

Q: The standard reduction potential of the permanganate ion, MnO4-, to Mn2+ is 1.51 volt, when it takes…

A: Redox potential is a measure of the tendency of a chemical species to get reduced, by accepting…

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: Metallic magnesium can be made by the electrolysis ofmolten MgCl2. (a) What mass of Mg is formed by…

A: (a) Mass formed by passing current can be given as: M: mass formed by metal on passing current.…

Q: A constant current of 5.29 amperes is passed through a cell containing In(NO3)3 for 5.75 hours. How…

A: Faraday law of electrolysis :- In accordance with Faraday law of electrolysis mass deposited or…

Q: A current of 4.88 A is passed through a Cu(NO,), solution. How long, in hours, would this current…

A: Given that  Current = 4.88 A = 4.88C/s  Mass of Copper diposited = 5.10g  Cu2+ + 2e- = Cu  1mol of…

Q: How many grams of mercury metal will be deposited from a solution that contains Hg* ions if a…

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Q: A current of 5.03 A is passed through a Cu(NO,), solution for 1.90 h. How much copper is plated out…

A:

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

A:

Q: (a) A Cr3+(aq) solution is electrolyzed, using a current of7.60 A. What mass of Cr(s) is plated out…

A: The mass of chromium deposited after two days can be calculated as follows-

Q: A current of 3.75 A is passed through a Sn(NO,), solution. How long, in hours, would this current…

A: Required time calculation for Electrolysis:

Q: Which species can be oxidized by Pb2+(aq)? Calculate the voltage for this/these process(es).

A: In the electrochemical series from Li (-ve Standard reduction potential) to F (+ve standard…

Q: A current of 4.26 A is passed through a Fe(NO,), solution. How long, in hours, would this current…

A: In Fe(NO3)2 the oxidation state of Fe is +3,and it gets reduced to Fe,i.e Fe gets deposited which…

Q: How many seconds are required to deposit 0.136 grams of copper metal from a solution that contains…

A: Given, mass of Cu deposited = 0.136 g Current passed = 0.913 A 1 Faraday is the magnitude of charge…

Q: (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell…

A:

Q: The standard hydrogen electrode (SHE) is used to produce a standard cell potential of exactly 1 V.…

A: The standard hydrogen electrode, is a oxidation - reduction electrode which is the base line of the…

Q: A galvanic cell consists of Mg anode in a 1.0 M Mg(NO,), and Al cathode in a 1.0 M AI(NO,), solution…

A: Concept is based on Electrochemistry Galvanic cells.

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

A: Given : Mass of Cr produced = 13.7 g And time = 90 min = 90 X 60 = 5400 s…

Q: 3) How many minutes will it take to plate out 16.22 g of Al metal from a solution of AS using a…

A: Given  Mass of Al =16.22g  Used Current =13.8amps Number of electrons =3 electrons (Al-->Al+3)…

Q: A current of 4.48 A is passed through a Fe(NO,)2 solution. How long, in hours, would this current…

A: Given, Amperes of current passed =4.48 A Solution = Fe(NO3)2 Iron plated = 6.30 g

Q: Calculate the enuilibrium constant for the following reaction using the standard half-cell…

A: In order to calculate the equilibrium constant we first write down the given data: T=298K. E0 for…

Q: How many seconds are required to deposit 0.221 grams of cadmium metal from a solution that contains…

A:

Q: (a) A Cr* (aq) solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out…

A:

Q: How many minutes will take to deposit 40.00 g of Ni form a solution of NiSO4 using a current of…

A: Faradays first law of electrolysis – During electrolysis of any material, the amount of material…

Q: How many grams of zinc metal will be deposited from a solution that contains Zn2+ ions if a current…

A: According to Faraday law:-     1F or 96485 c change passes to deposite equivalent mass of any…

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: Tollowing uld resuit for any CE aised from 25 °C to 100 °C? . The cell potential would not change at…

A: To discuss the Effect of temperature on the cell potential

Q: How many hours will it take to plate out all the copper in 250 ml of a 0.250 M Cu+ solution using a…

A:

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 seconds are required to deposit 0.107 grams of copper metal from a solution that contains…

A: Given data is as follows: The mass of copper metal = 0.107 grams The current applied = 0.903 A The…

Q: In the electrolysis of a solution containing Ag* (aq), metallic Ag(s) deposits on the cathode. Using…

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Q: When an aqueous solution of CuSO, is electrolyzed copper metal is deposited. If a constant current…

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Q: A current of 5.26 A is passed through a 2Sn(NO3)2 solution. How long, in hours, would this current…

A: In Sn(NO3)2 we have Sn in Sn2+ form  Hence to get tin that is Sn from Sn2+ the reaction will be Sn2+…

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.