How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr3+ ions for 40 minutes?

Q: 7. A current of 1000. A flows for exactly 1 hour, through a cell in which the following reaction…

A: Electric current : It is defined as the rate at which a particular charge flows. It is represented…

Q: How many seconds are required to deposit 0.189 grams of manganese metal from a solution that…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: How long will it take to plate out 3.9 g Ni from aqueous Ni2+ with a current of 108.2 A? HOW DO WE…

A: To plate Ni using the process of electrolysis, the reaction that needs to be employed on the…

Q: an acidic solution containing BiO+ is electrolyzed using a current of 0.500 A. what weight of Bi…

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

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

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: How many minutes will it take to plate out 40 g of Ni from a solution of NISO4 using a current of…

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Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

Q: How many grams of gold will be plated out by a current of 0.35 A applied for 65 minutes from a…

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

A: Faradays first electrolysis Law states that the quantity of reaction taking place in terms of mass…

Q: 1. What mass of the following substances can be produced in 1.0 h with a current of 15 A? a. Co from…

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Q: How long would it take to electroplate all the Zn^ 2+ in 0.280 L of .210 M ZnSO 4 solution with a…

A: The question is based on the concept of electrochemistry. It involves  application of first law of…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.05 minutes for a current of 1.91 A to plate…

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Q: How many grams of magnesium metal will be deposited from a solution that contains Mg2+ ions if a…

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Q: A constant current of 9.25 amperes is passed through a cell containing iridium (III) nitrate,…

A: We have current as 9.250 A , time as 7.57 hrs, deposit of Ir is taking place, we have to calculate…

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

A:

Q: How many seconds are required to deposit 0.268 grams of iron metal from a solution that contains…

A: Given  Mass deposited (m) = 0.268 g Current (i) = 1.22 A Time (t) = ? S The equation is Fe2+ + 2e-…

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

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

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Q: Calculate the mass of silver deposited at the cathode during electrolysis when a current of 1.80A…

A: Given that , Current (I) = 1.80 A Time (t) = 45 min = 45 x 60 = 2700 sec Electro chemical equivalent…

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

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Q: How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with a current of 105.9 A? HOW DO WE…

A: Given: Mass of Ni to be plated out = 1.0 g. Current pass = 105.9 A.

Q: A solution containing a 3+ metal ion is electrolyzed by a current of 5.0 A for 10 minutes. What is…

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

A:

Q: Calculate the mass in grams of a metal Q ( Molar mass= 88.23 g/mol) that will be deposited from a…

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Q: Determine the molar mass (amu) of Metal (M) if it took 2.85 minutes for a current of 1.1 A to plate…

A: Molar mass can be calculated as:-

Q: Gold can be plated out of a solution containing Au3+ according to the half-reaction:Au3+(aq) + 3…

A: It is given that gold is plated for 25 minutes and the current is of 5.5 A and the half-reaction is…

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

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Q: Gold can be plated out of a solution containing Au3+ according to the following half-reaction: Au 3+…

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Q: How many grams of tin metal will be deposited from a solution that contains Sn2+ ions if a current…

A: The metal deposited or liberated is given by the Faraday's first law of electrochemistry which is…

Q: How many grams of iron metal are plated out when a constant current of 8.50 A is passed through…

A: We have 8.5 A of current, passed for 50 minutes, we have to calculate the mass of iron metal…

Q: How many grams of metal Ca (40.08g/mol) are produced by electrolysis of CaBr2 using a current of 28…

A: Kindly get the answer given below.

Q: How many minutes would it take to plate 12g of silver from an aqueous Ag(l) solution using a current…

A:

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: How many grams of tin metal will be deposited from a solution that contains Sn2+ ions if a current…

A: The mass of metal deposited can be given by Faraday's first law of electrochemistry which is -  W =…

Q: How many grams of silver will be deposited by a current of 5.00A flowing through a cell for 10.0…

A:

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

A:

Q: In an electrolytic cell, how many grams of nickel (MM = 58.69 g/mol) will be deposited on a metal…

A: we have to calculate the mass of Ni deposited

Q: How long (hr) must a constant current of 50.0 A be passed through an electrolytic cell containing…

A: Answer: 5.36 hr

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

A:

Q: How many grams of  zinc metal will be deposited from a solution that contains  Zn^2+ ions if a…

A: In this question, we will determine the mass of Zn metal which is deposited from the Solution in…

Q: In the electrolysis of molten MgCl 2, what mass of Mg metal is deposited by a current of 16 amperes…

A: Electrolysis is the process of conversion of electrical energy to chemical energy. This reaction…

Q: How long would it take to produce 3.6 g of platinum by passing a 2.0 ampere current through a…

A: The mass of the substance (m) deposited or liberated at any electrode is directly proportional to…

Q: If in using a lead-acid battery to start a car, 1.00 gram of Pb (207.2 g/mol) is consumed on the…

A: Given:  m = 1 g of Pb MW = 207.2 mol = 1207.2= 0.004826 mol of Pb I = 0.5 C/s

Q: How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through…

A: Concept:  We have the charge given in form of the current and time taken, from Chemical equation of…

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: If a current of 15 A is run through an electrolysis cell for 2.0 hours, how many moles of electrons…

A: First find number coulombs (C) charge  i.e  Q = i x t  Where  Q= charge in coulombs  i = current  in…

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.