What mass of Ni metal can be plated on to the cathode from a NiSO4 solution using a current 8A for 15 minutes? (Atomic weigh for Ni is 58.71 amu)

Q: If a constant current of 2.0 amperes is passed through a cell containing Cr3+ for 1.0 hour, how many…

A: Mass of Cr deposited can be calculated using Faraday's first law of electrolysis: Mass deposited=…

Q: A solution of a metal ion ?(??) 3+ is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19…

A: The current transfered in the cell=5ATime for which the current is passed in the cell is 10minWe…

Q: Metallic Magnesium can be made by the electrolysis of Molten MgCl2. What mass of Mg is formed by…

A:

Q: 3. A factory wants to produce 1.0 x 103 kg Barium from the electrolysis of molten barium chloride.…

A: The given values are: m=1.0×103 kg=1.0×106 gt=4.0 h=4.0 ×3600 s The electrolysis step to form barium…

Q: Which electrode is the cathode? a Ag O b NO3 Na*

A: In a voltaic cell, the oxidation and reduction of metals occurs at the electrodes. The cathode is…

Q: An aqueous solution of nickel acetate is electrolyzed for 3 hours with a 1.3 ampere current. What…

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

Q: A steady current of 10 A maintained for 1 hr deposits 12.2 g of zinc at the cathode. What is the…

A: Given,  I = 10 A.  t = 1 hr.  m = 12.2 gm.

Q: Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold…

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Q: ii) How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce…

A: Use the first law of Faraday.

Q: Magnesium bars are connected electrically to underground iron pipes to serve as sacrificial…

A: Electrochemical cell is defined as the cell in which chemical energy is converted to electrical…

Q: What mass of Mg is formed by passing a current of 129 A through molten MgCl2, for 9.50 days?

A: Reaction-  Mg2+ + 2 e- ------------> Mg(s)

Q: In one process used for electroplating silver, a current of 10.23 A was passed through an…

A: Dear student, this question is related to electroplating process.

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: How much time in minutes would it take to deposit 1.65 grams of X (MW = 68.43 g/mol) on a cathode in…

A:

Q: How long, in minutes, will it take to produce 370.0 g of pure lithium by running a current of 330 A…

A: Given, Current passing = 330 A Mass of Li = 370.0 g  Molar mass of Li = 6.94 g/mol

Q: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that  An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

Q: A solution containg 75.0 mg copper was electrolyzed at a constant current of 0.250 A, causing…

A: Faraday's first law :  The amount of substance deposited is directly proportional to quantity of…

Q: 4. What current is required to deposit on the cathode 5.00 g gold/h from a solution containing a…

A: Current = Charge/Time  Q = I/t  1F =96500 C/mol  Mass of 1 mole =Molar mass

Q: ) In the electrolysis of a 200 mL unknown metal solution, 0.0434 grams of cathode mass increases…

A: We have given that  Volume of solution = 200mL  Mass deposited at cathode = 0.0434g  Current = I =…

Q: What is the time required to produce 45.0 g of Cl2 gas from Cl- using 50.0 A of current?

A: The oxidation reaction taking place will be  2 Cl- -------> Cl2 + 2 e-  Given : mass of Cl2 to…

Q: If a constant current of 2.0 amperes is passed through a cell containing Cr³+ for 1.0 hour, how many…

A: Given-> Current (I) = 2.0 ampere Time (t) = 1.0 hour = 1.0 × 60× 60 second = 3600 s Atomic mass…

Q: How much current should pass through

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Q: Suppose that a machine part requires 400 mg of copper to provide a coating that is thick enough for…

A: Given data,Current=0.5ATime=10min=10×60s=600s

Q: How many moles of hydroxide ion will be produced at the cathode during the electrolysis of water…

A: The given cathode reaction is: 2H2O + 2e- → H2 + 2OH- The balanced equation shows that for every 2…

Q: A solution of CuSO4 is electrolysis for 10 minutes with a current of 1.5 amperes. What is the mass…

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Q: What mass of gold is produced when 14.9 AA of current are passed through a gold solution for 28.0…

A:

Q: If an electrolysis plant operates its electrolytic cells at a total current of 150. A, how long, (in…

A: According to Faraday's First Law of Electrolysis, The amount of product deposited is directly…

Q: If a constant current of 7.3 amperes is passed through a cell containing Cu²+ for 1.5 hours, how…

A:

Q: What current in ampere will be required to produce 2.369 x10-3 kg of cu from CuSO4 solution in one…

A: Required mass of Cu to be produced = 2.369×10-3 Kg = 2.369 g Time given = 1 Hour = 1×60×60 = 3600…

Q: ow many grams of X (MW = 44.20 g/mol)(in g) will be deposited on a cathode in 1.91 h by a current of…

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Q: A factory wants to produce 1.0 x 10³ kg Barium from the electrolysis of molten barium chloride. What…

A:

Q: A galvanic (voltaic) cell contains a copper cathode immersed in a copper(II) chloride solution and a…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Metallic Magnesium can be made by the electrolysis of Molten MgCl2. What mass of Mg is formed by…

A: Given;

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.