How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for 2.00 h? (F = 96,500 C/mol)

Q: A solution of NaCl in water was electrolyzed with a current of 6.51 A for 23.0 min. How many…

A: Answer:Here:

Q: A current of 3.37 A is passed through a Cu(NO3)2Cu(NO3)2 solution for 1.30 h. How much copper is…

A: Given, the current = 3.37 A Time = 1.30 hour Now change the current (From A to C/s) and time (min…

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

A: Faraday's Law: It can be defined as by saying that the amount of substance produced at each…

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

A: Electroplating is a process in which a thin layer of one metal is deposited on another metal surface…

Q: How many seconds will be required to produce 1.00 g of nickel metal (58.693 g/mol) by the…

A:

Q: How many grams of copper metal can be deposited from Cu2*(aq) when a current of 2.50 A is run for…

A: current =2.50 A Time = 1.90 hours  The calculation of the amount of charge is as follows: Charge =…

Q: How many grams of aluminum metal will be deposited from a solution that contains Al3+ ions if a…

A: Answer : We have to calculate weight deposited in grams . Explanation : Al3+(aq) + 3e- -> Al(s)…

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 of 2.90 A was applied to an electrolytic cell containing molten CdCl2 for 54 minutes.…

A: We have to calculate the mass of cadmium metal deposited when current passed is 2.90 A for 54…

Q: How long will it take to plate 2.5 g of copper onto a light fixture using a solution of Cu(NO3)2 and…

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: 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: In a certain electrolysis experiment involving Al" ions, 50.4 g of Al is recovered when a current of…

A: Given data : In a certain electrolysis experiment involves Al3+ ions  50.4 g of Al is recovered by…

Q: A metal was galvanized with zinc using a solution of zinc nitrate, Zn(NO3)2. How much time was…

A: Answer :  We have to calculate time to plate zinc on the metal . Using Faraday laws of electrolysis…

Q: A current of 4.05 A is passed through a Cu(NO3)2 solution for 1.70 h. How much copper is plated out…

A:

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: A current of 0.46 A was passed through a copper (II) sulfate solution using copper electrodes for 16…

A: According to faraday law of Electrolysis:

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

A: Given, Current flow (I) = 8.15mA = 8.15×10-3A Time = 12.6 min = 756S 2I–(aq) → I2(aq) + 2e(Anode…

Q: Copper is electroplated from CuSO4 solution. A constant current of 5.79 A is applied by an external…

A:

Q: Gold is electroplated from Au(NO3)3 solution. A constant current of 3.14 amp is applied by an…

A:

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

A:

Q: Suppose that 4.29 g of a silver salt (AgX) is dissolved in 520.0 mL of water. A current of 3.46 A,…

A: we have to calculate the mass percentage of silver in the salt.

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.