If a constant current of 115 A is applied for 15.0 hours to the plating of cobalt from a cobalt(III) sulfate solution, how many grams of cobalt are plated during this time?

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

A: Ans is 0.546g

Q: A constant current of 1.6 A is used to precipitate copper at the cathode and oxygen at the anode of…

A: value of constant current = 1.6 A Time = 30.4 minutes cathode - copper Anode - oxygen

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

A:

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…

A:

Q: An aqueous solution of gold nitrate is electrolyzed with a current of 0.555 ampere until 1.32 g of…

A: The relationship between charge (q), time (t), and current (I) can be given as: q=I×t…

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

A:

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 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: 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: How many seconds are required to deposit 0.266 grams of cadmium metal from a solution that contains…

A:

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

A:

Q: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

A: We will calculate the standard reduction potential at 25 degree centigrade.

Q: In an experiment similar to this one, a polished strip of Cu (s) was found to weigh 16.552 g. This…

A: Given : Mass of Cu before electrolysis = 16.552 g Current passed = 0.887 A Time = 26 min = 26 X 60 =…

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

A:

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

A:

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

A:

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

A: Mass of cobalt is calculated as:-

Q: Determine the molar mass (amu) of Metal (M) if it took 2.95 minutes for a current of 1.8 A to plate…

A:

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

A: Mass can be calculated as:-

Q: How many seconds are required to deposit 0.136 grams of copper metal from a solution that contains…

A: Given, mass of Cu deposited = 0.136 g Current passed = 0.913 A 1 Faraday is the magnitude of charge…

Q: An aqueous solution of PdCl,2 is electrolyzed for 83.4 seconds and during this time 0.1064 g of Pd…

A:

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

A: Given: Time = 3.3 hours Current = 17.8 A Atomic mass of copper = 63.5 g/mol

Q: A current of 0.4 Amps flows for 2 hours through an electrolytic cell containing copper sulphate…

A: This problem can be solved by using Faraday's first law of electrolysis accordingto which weight of…

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

A:

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

A:

Q: How many seconds are required to deposit 0.221 grams of cadmium metal from a solution that contains…

A:

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

A:

Q: A constant current of 0.50 A is used to deposit copper at the cathode and oxygen at the anode of an…

A: Current = 0.50 A  Time = 10 minutes  F = 96485 C  Molar mass of copper = 63.55 g/mol  Weight of…

Q: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M1.0…

A: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M1.0…

Q: An engineer is assigned to design an electro chemical cell that will deliver a potential of exactly…

A: Given information: Cell potential = 1.52 V

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

A:

Q: How many seconds are required to deposit 0.252 grams of tin metal from a solution that contains Sn2*…

A: Mass of Sn = 0.252 g  Time = ?

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: 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: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

A: Answer is explained below.  For the given problem oxidation reaction, reduction reaction and the net…

Q: A current was passed for 5 hours through two electrolytic cells connected in series. The first cell…

A: Chemical equations for the reduction of gold and copper ions are: Au3+(aq)+3e-→Au(s)…

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: 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…

Q: How many seconds are required to deposit 0.150 grams of tin metal from a solution that contains Sn2+…

A: Mass = 0.150 g Current (i) = 0.652 A = 0.652 C/s  Time (t) = ?

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.