How much current is required to electroplate a metal surface with 0.493 g nickel metal from a solution of Ni2+(aq) in 811 seconds? Please provide full explanation.

Q: Copper metal can be purified electrolytically according to the following arrangement. The anode is…

A: W = I × t × M / n × F Where ; W = mass of  purified Cu = ? I = current = 15 A  t = time = 8.5 hours…

Q: How many grams of silver will be obtained when the aqueous silver nitrate solution is electrolyzed…

A:

Q: Using the standard reduction potentials listed in Appendix E, calculate the equilibrium constant for…

A: The standard reduction potential of oxidation half cell and reduction half cell

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

A:

Q: Consider the following standard reduction potentials:   Fe3+(aq) + e- → Fe2+( aq)…

A: Electrode reduction potential of all the species are there in a series which is known as…

Q: How many minutes will it take to electroplate 42.1 g of gold by running 5.00 A of current through a…

A: In an electrolytic cell for the electrolysis of a metal conversion of electrical energy in to…

Q: What volume of chlorine gas at standard temperature and pressure is evolved when a solution of MgCl2…

A: Provided time=1hour Molar mass of Cl2=70.906g/mol Let w gram Cl2 evolve So provided time…

Q: The following electrochemical data may be helpful in answering the question below. Use the table of…

A: Current (i) = 2.1 Ampere Weight of Cr = 0.8 gm

Q: (a) How long (in hours) does it take to produce 454 g of copper from a solution containing Cu²*…

A: Given: The mass of copper to be produced from Cu2+ = 454 g We have to find the amount of energy (in…

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: What mass (in g) of each product is produced in each of the following cells used for the…

A: "Since you have posted multiple questions, we will provide the solution only to the first two…

Q: In an electroplating cell, a metal ring was to be electroplated with silver. A current of 0.300 A…

A: Recall the following expression           WAg=EItF             Ag++e-→AgHere equivalent weightE of…

Q: How many grams of iron metal will be deposited from a solution that contains Fe* ions if a current…

A:

Q: How many milligrams of hydrogen can be produced by the electrolysis of water with a current of 0.308…

A: The electrolysis of water reaction producing hydrogen is  2 H+ + 2 e- -----> H2  Hence we can see…

Q: How many grams of manganese metal will be deposited from a solution that contains Mn2+ ions if a…

A:

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: 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: Chrome is plated from solutions of chromium(III) ions. If a particular application requires 13.7g of…

A: Given : Mass of Cr produced = 13.7 g And time = 90 min = 90 X 60 = 5400 s…

Q: How many seconds are required to deposit 0.175 grams of cadmium metal from a solution that contains…

A:

Q: Chromium is electroplated industrially by the electrolysis of solutions of K2Cr2O7. How much time…

A: A numerical problem based on electrolysis that is to be accomplished.

Q: A current of 3.68 A is passed through a Sn(NO3)2 solution. How long, in hours, would this current…

A:

Q: How many grams of copper will be plated out by a current of 2.3 A applied for 35 minutes to a 0.50 M…

A: ·  change(Q)=current(i)×time(t)· 1F change passed to cu2+ solution to deposite…

Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: Feasibility of redox reactions are expressed using their cell potentials which in turn computed…

Q: How long will it take to deposit 0.0047 mol of gold by electrolysis of KAuCl4 using a constant…

A:

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.