Calculate Current or Time How many amperes are required to deposit 0.242 grams of silver metal in 438 seconds, from a solution that contains Ag+ ions? How many amperes are required to deposit 0.188 grams of magnesium metal in 817 seconds, from a solution that contains Mg2+ ions? How many seconds are required to deposit 0.152 grams of copper metal from a solution that contains Cu2+ ions, if a current of 0.845 A is applied?

Q: How many seconds are required to deposit 0.137 grams of zinc metal from a solution that contains…

A: Mass of metal = I t × Mole Ratio × Atomic masd of metal / 96500  Where I = current  t = time

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…

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Q: How many minutes will it take for a current of 10.4 A to deposit 4.06 g of gold from a solution of…

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Q: A current of 4.76 A is passed through a Fe(NO3)2 solution for 1.20 h. Calculate the charge that…

A: Current = 4.76 A Time = 1.20 h

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

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Q: Suppose a current of 680. mA flows through a copper wire for 104. seconds. Calculate how many moles…

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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: current of 4.39 A is applied to a CuSO4 solution to deposit copper. Calculate the time it will take…

A: Given that: Current(I) = 4.39A = 4.39 C/s Mass of copper deposited = 1.00×102g = 100g

Q: How many seconds are required to deposit 0.224 grams of manganese metal from a solution that…

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Q: How long in seconds would it take to deposit 59.07 g of Pt from an aqueous solution of Pt 2+ with a…

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

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Q: Calculate the mass of Ag metal generated when Ag(NO3)(aq) is electrolysed for 20.5 minutes with a…

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

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Q: Enter your answer in the provided box. A constant current is passed through an electrolytic cell…

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Q: Determine the current (in A) to produce 6.50 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

A: Given information  Mass of Ag = 6.50 g Time = 2.00 h To calculate: Current

Q: an irregularly shaped metal part was made from a particular alloy was galvanized with zinc using a…

A: Given The amount of current (I) is 2.15 A The time is 2.2 hours The density of zinc is 7.410 g/cm3…

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: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: 1 F = 96500 C  Moles of chlorine = 1090 / 71 = 15.35 moles  Total charge = 2 × 15.35  F = 2 × 15.35…

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 chromium metal are plated out when a constant current of 8.00 A is passed through…

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Q: A current of 4.30 A is passed through a Pb(NO3)2 solution for 1.80 h. How much lead is plated out of…

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Q: Calculate the mass in grams of a metal Q ( Molar mass= 88.23 g/mol) that will be deposited from a…

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

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Q: In the electrolysis of an acid solution, oxygen can be produced by the following half-reaction:…

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Q: How many grams of nickel metal can be plated from 1.00M NISO4(aq), using a current of 3.00 A for…

A: Here mass of metal is calculated by using faraday's law

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: How many seconds are required to deposit 0.145 grams of zinc metal from a solution that contains Zn*…

A: Answer :-  t = 447 (s) The time required to deposit 0.145 g of Zn metal from a Zn2+ solution when…

Q: How many hours are required to plate 12.00 g of nickel metal from 1.00 M NİSO4(aq), using a current…

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Q: How many seconds are required to deposit 0.177 grams of manganese metal from a solution that…

A: Approach to solving the question: Detailed explanation: Examples: Key references:

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

A: We have given that  How many grams of magnesium metal will be deposited from a solution that…

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 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

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.