A baby’s spoon with an area of 6.25 cm2is plated with silver from AgNO3 using a current of 2.00 A for two hours and 25 minutes. (a) how many grams of silver are plated? (b) What is the thickness of the silver plate formed (d = 10.5 g/cm3)?

Q: An unknown metal M forms a soluble compound, M(NO3)3. A solution of M(NO3)3 is electrolyzed. When a…

A: The deposition is M+3 (aq) + 3e– ------> M (s)Number of moles of electrons = 3 × number of moles…

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 3.12 A3.12 A is passed through a Sn(NO3)2Sn(NO3)2 solution for 1.20 h1.20 h. How much…

A:

Q: 3. (a) Liquid NH3 is subjected to electrolysis. One of the half-reactions is 2 N3 N₂+6 e How many…

A: Given data:The given reaction is :a) How many faradays of electricity are required to produce 4.12 L…

Q: A current of 5.26 A is passed through a Pb(NO3)2 solution for 1.20 h. How much lead (in g) is plated…

A:

Q: How many minutes are required to deposit 1.39 g Cr from a Cr³⁺(aq) solution using a current of 2.50…

A:

Q: Three electrolytic cells are connected in a series. The electrolytesin the cells are aqueous…

A: The given data contains, current = 2.33 A. Mass of Cu = 1.74 g.

Q: Copper is electroplated from CuSO4 solution. A constant current of 4.28 A is applied by an external…

A:

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

A:

Q: According to the reaction, Ag+ (aq) + e- --> Ag(s), silver is deposited. For 30.0 minutes, a 0.800A…

A:

Q: How many grams of zinc, Zn (s) are electroplated out of a solution containing Zn2+ (s the solution…

A:

Q: How long would it take to deposit 3.75 g of iron from an aqueous solution of iron (III) sulfate by…

A: According to Faraday's First Law of Electrolysis, the chemical deposition due to flow of current…

Q: A current of 4.15 A is passed through a Pb(NO3)2 solution for 1.50 h. How much lead is plated out of…

A: Given that:  Current(I) = 4.15A = 4.15C/s  Time(t) = 1.50h = 1.50h×3600s/h = 5400s Reaction:  Pb2+ +…

Q: How long will an electrolytic cell containing a solution of cadmium(II) iodide need to run at a…

A:

Q: A current of 5.83 A is passed through a Fe(NO3)2 solution for 1.60 h. How much iron is plated out of…

A: According to Faraday's law of electrolysis, the amount of substance deposited on an electrode is…

Q: What current must be supplied to deposit 4.77 g of gold from a solution of AuCl 3 in 27.2 min?

A:

Q: A current of 9.22×104 A is passed through an electrolysis cell containing molten CaCl, for 10.9…

A: We will use relation of mass and gm equivalent

Q: A constant electric current flows for 3.55 h through electrolytic cells connected in series. One…

A: According to the Faraday's  first law of electrolysis Deposition of an element  due to the flow of…

Q: (a) Liquid H2O is subjected to electrolysis. One of the half-reactions is 2 H2O → O2 (g) + 4 H+(aq)…

A: We have to calculate the Faraday of electricity required and the time taken.

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: How many seconds are required to deposit 0.128 grams of magnesium metal from a solution that…

A:

Q: What volumes of H₂(g) and O₂(g) at STP are produced from the electrolysis of water by a current of…

A: Given ,

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: A current of 4.63 A4.63 A is passed through a Pb(NO3)2Pb(NO3)2 solution for 1.30 h1.30 h. How much…

A: Amount of substance deposited at electrode during electrolysis can be calculated as follows

Q: 2. (a) A voltaic cell is constructed as follows: Zn | Zn²+ | H*|H₂ The half-cell reactions are: Zn →…

A: The objective of the question is to find the concentration of H+ ions, the pH of the cathodic…

Q: Metallic iron can be made by the electrolysis of molten Fe2O3. (a) What mass of Fe is formed by…

A:

Q: What mass of each of the following substances can be produced in 1.2 h with a current of 11 A? (a)…

A: Current = 11 ATime = 1.2 h

Q: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

A: According to Faraday's 1st law weight of the substance from in each electrolyte  W = ZIt where , W…

Q: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

Q: This is an example of a disproportionation reaction:…

A:

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

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.