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: (a) Write the half-reaction that occurs at a hydrogen electrode in acidic aqueous solution when it…

A: Concept introduction: Anodic reaction: It is the reaction that occurs at anode by loss of electrons…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.21 minutes for a current of 1.24 A to plate…

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

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

A: Amount of charge (Q) = I . t  where I = current and t = time

Q: Let’s say that you want to plate gold metal on the outside of some heart pendants (to give to all of…

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…

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Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to…

A: Equivalents of H+ ions reduced = QF=I×t96500=11.3 ×73 ×6096500= 0.513 Total equivalents of H+ ions…

Q: (a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a…

A: i = 81.2 A t = 59.2 min

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: (19) Consider the following redox reaction that occurs in a voltaic cell: Cr2+ (aq) + Cu2+ (aq) →…

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Q: What mass of zinc (in grams) is deposited at the cathode when a current of 9.8 amperes passes…

A: According to the electrochemistry Mass of substance deposited,  W = ZCt Where,   t = time in second…

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

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Q: Determine the molar mass (amu) of Metal (M) if it took 1.04 minutes for a current of 1.22 A to plate…

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

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

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

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Q: Determine the current (in A) to produce 3.10 g Ag when Ag"(aq) is electrolyzed for 2.00 h. (F =…

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Q: A silver material is to be plated with gold using an aqueous solution of Au*3. How many moles of…

A: we have to calculate moles of gold deposited

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…

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Q: You want to design a galvanic cell using an iron (Fe) electrode as the cathode. Which of the…

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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: A Cr3+1aq2 solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out…

A: Charge flowing per unit time is known as current which may be expressed mathematically as :…

Q: 2+ A current of 3.40 A is passed through a solution containing Cu²+ (aq) for 30.0 minutes, with…

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

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Q: How many grams of Ag can be produced by passing a current of 0.350 A through a solution of AgNO3 for…

A: Faraday first law of electrolysis:  The mass of substance (m) deposited at an electrode is directly…

Q: 12) What mass of silver can be plated onto an object in 67 minutes at 8.70 A of current? Ag'(aq) + e…

A: Given ->  Time (t) = 67 minutes = 67 × 60 seconds= 4020 s  (1minute = 60 seconds)  Current (i) =…

Q: What mass of copper could be deposited from a copper(II) sulfate solution using a current of0.50 A…

A: The given problem can be solved by using the formula as; Q=I×t…

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

A: Mass can be calculated as:-

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: Nickel can be produced when a current is passed through an aqueous solution of nickel (II) acetate.…

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Q: Determine the molar mass (amu) of Metal (M) if it took 1.29 minutes for a current of 1.48 A to plate…

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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: 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…

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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: How many minutes would it take to plate 12g of silver from an aqueous Ag(l) solution using a current…

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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: 2. A Galvanic cell is constructed from a Cu*/Cu electrode and an Ag*/Ag electrode. (1) Make a…

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Q: Metallic magnesium can be made by the electrolysis of molten MgCl2. (a) What mass of Mg is formed…

A: Given chemical reaction is :  MgCl2 (s)  ---------->  Mg(s)  +  Cl2 (g)  It is a thermal…

Q: current of 2.505 A deposits 1.371 g of a metal M from a solution that contains the metal ion M²⁺ in…

A: Given, current (i) = 2.505 A Time (t) = 30 × 60 = 1800 s Mass = 1.371 g  Using Faraday's law,  Mass…

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

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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.