How many seconds are required to deposit 0.189 grams of manganese metal from a solution that contains Mn ions, if a current of 0.710 A is applied?

Q: How many seconds are required to deposit 0.274 grams of manganese metal from a solution that…

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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 0.600 A deposits 1.33 g of a certain metal in 1.00 hour. Assume a two-electron…

A: Given: 1.33 g is the weight of the metal deposited, 0.66 A is current, 1 hour is the time taken, and…

Q: How many minutes would be required to deposit 0.375g of calcium using a current of 3.93A?

A: Given,  Mass of Ca = w = 0.375 g  Current = I = 3.93 A  Time required = t = ?

Q: How many grams of nickel remains in a 100 ml of 1.50 M NİCI4 solution if 3.0 ampere current is…

A: V = 100 ml = 0.1 L M = 1.50 M I = 3 Amp t = 1 hr = 60 x 60 = 3600 sec W = ? nf = 4 By using Faraday…

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

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Q: How many y seconds are required to deposit 0.216 grams of silver metal from a solution that contains…

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Q: Copperplating is a technique in which copper metal is deposited electrolytically on a surface to…

A: The objective of this question is to calculate the time required to plate 1.50 g of copper metal…

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

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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: How many grams of mercury metal will be deposited from a solution that contains Hg2+ ions if a…

A: Given :  Current (I) = 0.599 A  Time(t) = 28.4 min = 28.4 x 60 sec = 1704 sec  Molar mass of Hg =…

Q: How many seconds are required to deposit 0.218 grams of tin metal from a solution that contains Sn2+…

A: F = 96500 C mol-1 Current = charge/time

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: the electromotive force of a galvanic cell constructed of a standard hydrogen electrode and a lead…

A: The electrode potential when the concentration of all the half cells involved is unity is called the…

Q: What mass, in grams, of pure potassium will be produced if a current of 358.5 A is run through a…

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

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Q: How many grams of nickel metal will be deposited from a solution that contains Ni²+ ions if a…

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Q: How many grams of silver metal will be deposited from a solution that contains Ag+ ions if a current…

A: Amount of current passed through the solution containing Ag+ ions = 0.695 A  Time of this current…

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

A: Given,

Q: Answers 1-10

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

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Q: How many grams of zine metal will be deposited from a solution that contains 2+ Zn ions if a current…

A: The charge is directly proportional to the current and time associated with it. According to…

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

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Q: How many grams of copper metal will be deposited from a solution that contains Cu2+ ions if a…

A: Here we use the formula of metal deposited= ZIt , where Z is molecular weight, I= current, t= time…

Q: How many grams of iron metal will be deposited from a solution that contains Fe* ions if a current…

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

A: I=0.785 amperes t=61.9minutes n = 2 w=ZIt = 65.3 × 0.785× 61.9 ×60 /2× 96500 w =0.986gm

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 milligrams of hydrogen can be produced by the electrolysis of water with a current of 0.308…

A: The electrolysis of water reaction producing hydrogen is  2 H+ + 2 e- -----> H2  Hence we can see…

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 manganese metal will be deposited from a solution that contains Mn2+ ions if a…

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Q: How many grams of manganese metal will be deposited from a solution that contains Mn2+ ions if a…

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Q: How many grams of iron metal will be deposited from a solution that contains Fe* ions if a current…

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

A: Weight of Mg deposited can be calculated using the equation of Faraday's first law. Answer is 0.2732…

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

A: The given data is as follows: The current applied (I) = 1.10 A The time (t) = 32.1 minutes = 32.1×60…

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

A: Faraday's first law of electrolysis states that during an electrolysis reaction the mass of the…

Q: How many seconds are required to deposit 0.166 grams of chromium metal from a solution that contains…

A: The mass of Chromium deposited from a Cr3+ ion solution is w = 0.166 g. The applied current is I =…

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

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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.