In an experiment similar to this one, a polished strip of Cu (s) was found to weigh 16.552 g. This strip was electrolyzed for exactly 26 minutes at an average current of 0.887 amps. The weight of the copper strip after electrolysis was 17.896 g. From these data, calculate the value of the Faraday constant.

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

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Q: A current of 0.600 A deposits 1.33 g of a certain metal in 1.00 hour. Assume a two-electron…

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A: Given  Current (i) = 0.25 amperes Time (t) = 10 hours  = (10×60×60) seconds  t = 36000 seconds  Mass…

Q: Purification of copper can be achieved by electrorefining copper from an impure copper anode onto a…

A: Current passed = 40 amp Mass of Copper to be deposited = 18.5 g Number of moles of Cu deposited =…

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A: Given: Current = 4 A Time = 10.0 min Electrochemical equivalent of silver is 1.1180 x 10– 6 kg/C

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Q: An electrolysis cell that deposits copper (from Cu2+ ions) operates for 30 minutes at an electric…

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Q: current of 4.39 A is applied to a CuSO4 solution to deposit copper. Calculate the time it will take…

A: Given that: Current(I) = 4.39A = 4.39 C/s Mass of copper deposited = 1.00×102g = 100g

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A: Here we have to determine cell voltage of the following given Galvanic cell. For this first we…

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: Answer:- This question is answered by using the simple concept of calculation of mass using the…

Q: How many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a…

A: The amount of metal deposited on electrode is given by Faraday's first law of electrochemistry,…

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A:

Q: How many grams of copper metal will be deposited from a solution that contains Cu2+ ions if a…

A: Given: Amount of current = 1.03 A Time duration = 28.4 minutes.

Q: An aqueous solution of AICI3 is electrolyzed for 1.50 hours producing 5.45 g of aluminum What is the…

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Q: One half-cell in a voltaic cell is constructed from a silver wire dipped in silver nitrate solution…

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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: What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for 143…

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Q: Purification of copper can be achieved by electrorefining copper from an impure copper anode onto a…

A: Answer: Faraday's first law of electrolysis states that mass of metal deposited during electrolysis…

Q: Fischl, a scientist from Mondstadt specializing in electrochemistry, performed an electrolytic cell…

A: Given Amount of metal deposited = 15.73 g Current = 1.5 A Time = 5 hours n = 2

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Q: Electrolysis of an NaCl solution with a current of 2.02 A  for a period of  205 s produced   59.2 mL…

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Q: impure

A: According to this law,  mass diposite on cathode is direactly proportion to the current.  So,…

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A: We have following reaction Ni2+ +2e ---> Ni(s) moles of electrons required to form 1 mole Ni(s)=2…

Q: what mass of platinum could be plated on an electrode from the electrolysis of a Pt(NO3)2 solution…

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Q: Purification of nickel can be achieved by electrorefining nickel from an impure nickel anode onto a…

A: This is a problem of electrochemistry.It is basically a study of the chemical processes that cause…

Q: Calculate the quantity indicated for each of the following electrolysis. a. The mass of Zn deposited…

A: The mass of zinc can be calculated by using Faraday's law of electrolysis.

Q: How long will it take to plate 2.5 g of copper onto a light fixture using a solution of Cu(NO3)2 and…

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Q: An electrochemical cell is constructed in which the silver ions in silver chloride are reduced to…

A: Given,  A current of 0.500 A is passed through the cell for 101 minutes. The mass of copper metal…

Q: e mass of pure aluminum produced.

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Q: A copper penny can be dissolved in nitric acid but not in hydrochloric acid. Using reduction…

A: We know that, Cu(s)→Cu+2(aq)+2e-                                                Eo=-0.34…

Q: How long (in minutes) would it take to deposit 0.67 g of copper from a solution containing Cu? using…

A: Faraday law of electrolysis      M = AnF×I×T            where,        M = mass of metal deposited…

Q: In a large number of samples of water, in which the copper ion concentration is expected to be quite…

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Q: When an aqueous solution of copper sulphate is electrolyzed, copper is deposited at the cathode…

A: Half-cell reaction for deposition of Cu is  Cu2+ + 2e- --> Cu Calculate the moles of Cu Mass of…

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: Chromium metal can be electroplated from an aqueous solution of potassium dichromate. The reduction…

A: Charge = current *time  Current = 5.5 A  Time = 46 minutes = 46*60 s = 2760 s  Charge = 2760*5.5 =…

Q: What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr,(SO)3 for 149…

A: From Faradays First law of electrolysis,  the amount of the substance deposited(W) at the given…

Q: Electrolysis can be used to purify silver.  What mass of silver would plate onto the pure electrode…

A: One Mole of electron = 96500 C

Q: Write the balanced equation for the overall reaction that occurs in the cell. Calculate E ̊ for the…

A: The reaction with smaller standard electrode potential, that reaction occurs at anode and reaction…