Calculate Current or Time How many amperes are required to deposit 0.242 grams of silver metal in 438 seconds, from a solution that contains Ag+ ions? How many amperes are required to deposit 0.188 grams of magnesium metal in 817 seconds, from a solution that contains Mg2+ ions? How many seconds are required to deposit 0.152 grams of copper metal from a solution that contains Cu2+ ions, if a current of 0.845 A is applied?

Q: How many seconds are required to deposit 0.274 grams of manganese metal from a solution that…

A:

Q: The MnO2 used in alkaline batteries can be produced by an electrochemical process of which one…

A: Answer: 174.0

Q: How long must constant current of 50.0 A be passed through an electrolytic cell containing aqueous…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: A constant current is passed through an electrolytic cell containing molten MgCl2 for 12 hours. If…

A:

Q: How many seconds are required to deposit 0.239 grams of manganese metal from a solution that…

A:

Q: How many seconds are required to deposit 0.224 grams of manganese metal from a solution that…

A:

Q: How long must a current of 20.0 amps be applied to a solution of CrCl3 to produce 175 g of Cr (s)…

A:

Q: What current is needed to deposit 0.500 g of chromium metal from a solution of Cr3+ in a period of…

A: The formula for the calculation is W= Z x I x t Where W = amount of chromium deposited(0.500g)…

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,…

Q: A metal object is to be gold-plated by an electrolytic procedure using an aqueous AuCla solution.…

A: Given : Time = 3.0 min = 3.0 X 60 = 180 s                                              (Since 1 min…

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A:

Q: Determine the current (in A) to produce 6.50 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

A: Given information  Mass of Ag = 6.50 g Time = 2.00 h To calculate: Current

Q: Using a constant current of 6.9 A, a metal object is to be gold-plated by an electrolytic procedure…

A: Consider the given information is as follows; Current (I) = 6.9 A Time (t) = 9.8 min = 9.8×60=588…

Q: Determine the current (in A) to produce 3.10 g Ag when Ag"(aq) is electrolyzed for 2.00 h. (F =…

A:

Q: n a copper plating experiment in which copper metal is deposited from a copper(II) ion solution, the…

A: Using Faraday's First of electrolysis: w = ZIt Z = Equivalent mass of metal96500w = Molar mass of Cu…

Q: A current of 0.500 A flows through a cell containing Cd(II) for 10.0 minutes. Calculate the maximum…

A: Current Strength = 0.500 A time = 10 min         = 10 × 60 sec                               (As, 1…

Q: Using a constant current of 7.8 A, a metal object is to be gold-plated by an electrolytic procedure…

A:

Q: A zinc bar (atomic mass = 65.38 g/mol; ion charge = 2) is weighing 2.4 kg is attached to a buried…

A: The solution is given below -

Q: When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes, the…

A: 8.15mA current flows which is equal to 0.00815A time is 12.6min = 756s The molar mass of I2 =…

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: The charge carried by one electron is 96500 C. The electrode reaction:

Q: Determine the current (in A) to produce 6.50 g Ag when Ag*(aq) is electrolyzed for 2.00 h. (F =…

A: The faraday's second law states that "when same amount of current is passed through different…

Q: How many seconds are required to deposit 0.239 grams of zinc metal from a solution that contains…

A:

Q: If a constant current of 115 A is applied for 15.0 hours to the plating of cobalt from a cobalt(III)…

A:

Q: Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature and…

A: It is given that MgCl2 is electrolysed and a current of 12.4 A is passed for 1h.

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

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

A: Here we use the formula of metal deposited= ZIt , where Z is molecular weight, I= current, t= time…

Q: How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through…

A: We have, Cr3+ needs 3 Faradays to plate 1 mole This means that for every 3 moles of electron…

Q: How many seconds are required to deposit 0.223 grams of lead metal from a solution that contains…

A: Given that, 0.223 grams of lead metal (Pb) is deposited from a solution that contains Pb2+ ions and…

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: Electrolysis is a process in which current is passed through a substance .In this chemical reactions…

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

A: Given:  Current = 0.974 A  Time = 67.4 min = 67.4 x 60 = 4044 sec

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: current

A:

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: The charge carried by one electron is 96500 C. The electrode reaction: Given that current passed is…

Q: current of 2.505 A deposits 1.371 g of a metal M from a solution that contains the metal ion M²⁺ in…

A: Given, current (i) = 2.505 A Time (t) = 30 × 60 = 1800 s Mass = 1.371 g  Using Faraday's law,  Mass…

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

A:

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

A:

Q: Electrolysis of an aqueous solution of sodium chloride produces chlorine, Cl, (g). The reaction that…

A:

Q: A galvanic cell runs for 1 minute with a current of 0.20 A. How much charge passed through the cell…

A: Given : Current passed = 0.20 A And time = 1 min

Q: What current is used to liberate 213 grams of chlorine, Cl 2 from a solution NaCl if it take 2…

A: Faraday's 1st law of electrolysis is one of the most important law which explains that the quantity…

Q: Which of the following statements associated with the pH meter is incorrect? (A) The pH meter should…

A: A question based on electrolysis that is to be accomplished.

Q: current of 6.6 A is passed through a solution of AgNO3 to electroplate it onto a surface. Calculate…

A:

Q: A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl3electrolyte.…

A: Welcome to bartleby! Introduction :  We have to calculate number of moles deposited .

Q: how many minutes are required to plate 10.0g of nickel metal from a solution of NiSO4, if the…

A:

Q: decided to deposit 55.00 g of gold over an iron medallion by electroplating it from a solution…

A:

Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for…

A: Given values:I = 0.912 ATime = 18.5 h It is known that 1 h = 3600 sec.Therefore, 18.5 h = 18.5×3600…

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

A: we know the expression for the faraday's law of electrolysis is => m/E = It / F Where,  m is the…

Q: A galvanic cell runs for 1 minute with a current of 0.25 A. How much charge passed through the cell…

A: Given : Current passed = 0.25 A And time = 1 min F=96500 C/mol

Q: Consider an electrolytic cell with a steady current of 174 amperes which produces Als) (atomic mass…

A:

Q: How long will it take to plate out 4.2 g Ni from aqueous Ni2+ with a current of 112.3 A? HOW DO WE…

A:

Q: How many grams of mercury metal will be deposited from a solution that contains Hg2+ ions if a…

A: Given: Current passed = 0.869 A  And time taken = 69.2 min = 69.2 × 60 = 4152 s…

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.