How many hours would it take to produce 72.9 g of metallic chromium by the electrolytic reduction of Cr+ with a current of 1.14 A? Time = |hr

Q: What is the value of equilibrium constant, Keq, for the reaction between copper metal and iron (III)…

A: When iron(III) react with copper reaction take place then iron(III) is reduced to iron(II)  and…

Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A: Ga3+ + 3e– ----> Ga(s)   Charge  = Current × time (s) = 0.830 A × (30.0 × 60 ) s = 1494 C

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

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Q: Calculate the mass of Li formed by electrolysis of molten LiCl by a current of 7.5 * 104 A flowing…

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Q: An aqueous solution of copper sulphate, CuS04 was electrolysed between platinum electrodes using a…

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Q: Given the following standard reduction potentials: Reaction A, E°red = 0.34 V Reaction B, E°red =…

A: Oxidizing reagent reduces it's self in the reaction,but oxidizes the Substrate in the reaction.  So…

Q: Please with complete solution and good penmanship

A: Dear student, this question is related to electrolytic cell.

Q: It took 116 hours to produce 603 g of metal X by performing electrolysis on molten XC13 with a…

A: From Faraday’s first law of electrolysis the quantity of charge is calculated as: Where, Q is…

Q: 1) Molten metal chloride (MC13) subjected to a current of 6.50 A for 0.388 hours deposits 1.41g of…

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Q: Two metals A and B have reduction potential values of –0.25V and 0.80V respectively. Which of these…

A: Given that: Reduction potential of metal A = -0.25 V Reduction potential of metal B = +0.80 V Which…

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: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A:

Q: Calculate the mass of nickel that will be deposited when a current of 2.00 A is passed through a…

A:

Q: If 2.19 g of chromium metal was deposited from a solution of Cr3+ using a current of 35.2 amps in an…

A: Given, If 2.19 g of chromium metal was deposited from a solution of Cr3+ using a current of 35.2…

Q: 1.) How many minutes will it take to plate out 2.19 g of chromium metal from a solution of cr" using…

A: 1. mass of Cr = 2.19 g  current = 35.2 A    Note : Since there are multiple questions, as per policy…

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below:…

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Q: hromium can be electroplated from aqueous potassium dichromate, with the reduction shown below:…

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Q: Calculate the concentration of Cu1+ needed to produce a galvanic cell containing Cu1+ and Cu (s)…

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Q: Thorium, Th, is an actinide metal that can be used as a contact explosive much solid thorium could…

A: Given, Current is passed through Th4+ solution is ---- 0.51A Time is ---- 3hours How much thorium is…

Q: A concentration cell similar to the one shown is composed of two Cu electrodes and solutions of…

A: Electrochemical cells are those which converts the chemical energy into the electrical energy. They…

Q: How many grams of chromium metal will be deposited from a solution that contains Cr ions if a…

A: By faraday's law of electrolysis, m=ZIt Here m is the mass of Cr3+ in grams. Z is electrochemical…

Q: What is the efficiency of an electrolytic cell that produces 20.0 g of elemental chromium from a…

A: Efficiency of an electrolytic cell means its current efficiency. The current efficiency is a ratio…

Q: 32. What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for…

A: Given that,time, t = 244.7 min = 244.7 x 60 sec = 14682 seccurrent, i = 13.6 A F = 96485…

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

A:

Q: What mass of Cu(s) is electroplated by running 12.5 A of current through a Cu 2+ (aq) solution for…

A: We have to calculate the mass of Cu(s) is electroplated : First, we will write down all the given…

Q: How much silver was in the solution if all the silver was removed as Ag metal by electrolysis for…

A: Applying Faraday law  W= Zit

Q: How many moles of chromium would be electroplated by passing a current of 5.2 amperes through a…

A: Charge = current *time  Time =2700s  Current =5.2 A

Q: A concentration cell similar to the one shown is composed of two Ni electrodes and solutions of…

A: In concentration cell same electrode and same substance is used in solution.The only difference is…

Q: If it is shown that titanium can be used as a sacrificial anode to protect iron, what conclusion can…

A: Sacrificial anodes are active metals which are used to avoid a less active material surface from…

Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

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Q: How many hours are required to produce 5.00 g of chromium metal from an acidic solution of potassium…

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Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A: Given that: current, I = 0.590 A  time =  90.0 min To find: amount of Ga(s) deposited from a…

Q: How many grams of nickel metal will be deposited from a solution that contains Ni2+ ions if a…

A: 1)  According to Faraday second Law :-     When 1 F or  96485 e change passes it deposite…

Q: 5. If 2.46 g of Fe 2+ were oxidized in the reaction Fe2+(aq) + Ce4+( aq ) à Fe3+ (aq) + Ce3+ (aq ),…

A: The molar mass Fe atom is:- 55.85g/mol

Q: Predict the products of the electrolysis of an aqueous solution of sodium chloride in cell using…

A: Electrolysis is a spontaneous redox process Here we are required to find the product when aqueous…

Q: Calculate the cell potential of tho following cell at 25°C. Cr(s) | C" (1.0 X 10° M) || Ni²* (1.5 M)…

A: Given data,[Cr3+]=1.0×10-3M[Ni2+]=1.5MTemperature=25oC

Q: How long, in hours, will it take to electrodeposit 181 g of aluminum in a cell with molten AICI3…

A: Given, mass of Al = 181 g Current (I) = 123 A Time (t) = ? Note: molar mass of Al = 27 g/mol

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Q: Calculate the mass (in grams) of K formed by a current of 6.5 x 104 A flowing for 24 hours if the…

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Q: How many seconds

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Q: A 10.0 gram sample of copper ore was dissolved in nitric acid and then electrolyzed until all of the…

A: Percentage of copper in the original sample can be calculated by knowing the amount of copper metal…

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: What volume of CL2 at 1 atm, 25 Co would be produced from the electrolysis of molten NaCl for 10…

A: Quantity of electricity can be calculated using the relation: Q = i × t Q = 7 Amps × 10 hr Q = 7…

Q: What mass of silver would plate onto the cathode if a current of 7.9 A flowed through the cell for…

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Q: How many minutes will it take to plate out 2.19 g of chromium metal from a solution of Cr3+using a…

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Q: How many grams of cadmium metal will be deposited from a solution that contains Cd²+ ions if a…

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Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A: We have to calculate the amount of gallium solid that can be formed.

Q: What is the change in mass (in grams) of the anode if a 19.00 A current runs for 11.40 h during the…

A: Electrolysis is the process of decomposing a substance into their components.  According to faradays…

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.