How many seconds would be required to produce 50.0 g of Mg from MgCl2 if the current is 100.0 A?

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

A: Ans is 0.546g

Q: How many seconds are required to deposit  0.207 grams of iron metal from a solution that contains…

A: According to Farady's law of electrolysis we can write m =I×t×MF×νwhereI = currentt = timeM = atomic…

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 seconds are required to deposit 0.167 grams of cadmium metal from a solution that contains…

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Q: How many minutes will it take to plate out 40 g of Ni from a solution of NISO4 using a current of…

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

A: The Faraday's 1st law of electrolysis is one of the most important law which explains the…

Q: How many seconds are required to deposit 0.239 grams of manganese 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: Given: Amount of current = 1.03 A Time duration = 28.4 minutes.

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

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

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Q: 10

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Q: mass of copper

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Q: How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with a current of 105.9 A? HOW DO WE…

A: Given: Mass of Ni to be plated out = 1.0 g. Current pass = 105.9 A.

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: Determine the current (in A) to produce 4.50 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

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Q: Determine the molar mass (AMU) of Metal (M) if it took 2.56 minutes for a current of 1.11 A to plate…

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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: The faraday's second law states that "when same amount of current is passed through different…

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

A: Mass of cobalt is calculated as:-

Q: How many seconds are required to deposit 0.239 grams of zinc metal from a solution that contains…

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Q: How many seconds are required to deposit 0.168 grams of lead metal from a solution that contains…

A: We have deposit of pb as 0.168g . Current passed is 0.974 A We have to calculate the time required…

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 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: What mass (in grams) of nickel could be electroplated from a solution of nickel(II) chloride by a…

A: From Faraday's first law of electrolysis, the weight of a chemical substance(w) deposited at an…

Q: How many seconds are required to deposit 0.270 grams of copper metal from a solution that contains…

A: Given weight of deposited copper metal from a solution(w) = 0.270 g  Current applied (I)= 0.828 A =…

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: How many grams of tin metal will be deposited from a solution that contains Sn2+ ions if a current…

A: The metal deposited or liberated is given by the Faraday's first law of electrochemistry which is…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.54 minutes for a current of 1 A to plate…

A: From combination of first and second law of Faraday, we have :  M = n*F*m/(I*t) ....(1) Here, n =…

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

A:

Q: How many grams of tin metal will be deposited from a solution that contains Sn2+ ions if a current…

A: The mass of metal deposited can be given by Faraday's first law of electrochemistry which is -  W =…

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

A: Reduction: It is a chemical reaction which is associated with an increase in the number of electrons…

Q: How many seconds are required to deposit 0.175 grams of cadmium metal from a solution that contains…

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Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: The mass of aluminum metal calculated as follows

Q: How many seconds are required to deposit 0.164 grams of magnesium metal from a solution that…

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Q: What period of time (in hours) is required to produce 1.00mol of chlorine using a current of 5.00A?

A: A numerical problem based on Faraday's law, which is to be accomplished.

Q: Determine the current (in A) to produce 3.00 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

A: The half reaction when Ag+ (aq) is electrolyzed.                                           Ag+ (aq)…

Q: How many seconds are required to deposit 0.278 grams of manganese metal from a solution that…

A: Electrical charge is defined as the multiplication of current and time. It is measured in coulombs.…

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

A: According to Faraday law:-     1F or 96485 c change passes to deposite equivalent mass of any…

Q: how many minutes are required to plate 10.0g of nickel metal from a solution of NiSO4, if the…

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

A: In this question, we will determine the mass of Zn metal which is deposited from the Solution in…

Q: How long will it take to plate out 4.9 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

A: Given:: Mass of Ni= 4.9 g molar mass of Ni=58.6934 g mol-1 charge = ?

Q: How long would it take to produce 3.6 g of platinum by passing a 2.0 ampere current through a…

A: The mass of the substance (m) deposited or liberated at any electrode is directly proportional to…

Q: How much time is needed to deposit 1.0 g of chromium metal from an aqueous solution of CrCl3 using a…

A: Faraday's law of electrolysis draws a relationship between the amount of substance deposited by an…

Q: How many seconds are required to deposit 0.150 grams of tin metal from a solution that contains Sn2+…

A: Mass = 0.150 g Current (i) = 0.652 A = 0.652 C/s  Time (t) = ?