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 lead is plated out of the solution?   mass of lead:

Q: Simply by living, an 87.5 kg human being will consume approximately 20.0 mol of 0, per day. To…

A:

Q: How long will it take to plate out 3.9 g Ni from aqueous Ni2+ with a current of 108.2 A? HOW DO WE…

A: To plate Ni using the process of electrolysis, the reaction that needs to be employed on the…

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

A:

Q: 1. What mass of the following substances can be produced in 1.0 h with a current of 15 A? a. Co from…

A:

Q: How long must a current of 20.0 amps be applied to a solution of CrCl3 to produce 175 g of Cr (s)…

A:

Q: A current of 11.8 A is applied to 1.25 L of a solution of 0.549 mol L- aqueous HBr converting some…

A:

Q: Consider an electrolytic cell where silver metal is plated (reduced) from an  aqueous silver nitrate…

A:

Q: Simply by living, an 87.5 kg human being will consume approximately 20.0 mol of 0, per day. To…

A: The answer is given below :

Q: Manganese metal can be produced industrially by electrolysis of MnO2. How many hours would it take…

A: The compound of manganese electrolysed is MnO2 having Mn4+ ion. Hence the electrolysis reaction to…

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: Manganese dioxide (MnO2) for use in dry cell batteries is made by electrolyzing solutions of Mn2*…

A:

Q: 5. Consider the following reactions: 3 Ni 2"taq) + 2Cr(OH)3 (s) + 10 OH ¯ (aq) → 3 Ni (s) + 2 CrO4…

A:

Q: 6. A 1M aqueous solution of chromium (I) bromide will be electrolyzed to "chrome plate" a faucet.…

A: As per the Faraday's 1st law of electrolysis: w=ZIt      ----(1)where,w = weight of the substance…

Q: A current of 3.86 A is passed through a Pb(NO,), solution for 1.60 h. How much lead is plated out of…

A: Faraday law of electrolysis states that the amount of substance deposited at the electrode is…

Q: A current of 0.500 A flows through a cell containing Cd(II) for 10.0 minutes. Calculate the maximum…

A: Current Strength = 0.500 A time = 10 min         = 10 × 60 sec                               (As, 1…

Q: a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

A: Given data: Current = 67.8 A = 67.8 C/sec Time = 86.4 min = 86.4 x 60 sec Formula used: q = I x t

Q: What mass (in grams) of nickel (AW = 58.69) could be electroplated from a solution of nickel(II)…

A: Given that:  Current(I) = 0.25A = 0.25C/s Time = 10 hours = 10h×3600s/h = 36000s

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

A: Since in the above reaction we can see that 1 mole of Cl2 is produced with 2 moles of electrons…

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: Consider the following cell reaction: Ni(s) + 2 H+(? M) Ni2+(1.00 M) + H2(g)(1.00 atm) If the cell…

A: cell potential at 298 K is 0.125 volt

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: Determine the molar mass (amu) of Metal (M) if it took 2.95 minutes for a current of 1.8 A to plate…

A:

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

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: Oxygen Supply in Submarines Nuclear submarines can stay under water nearly indefinitely because they…

A:

Q: An alternator recharges an automobile battery when the engine is running. If the alternator produces…

A: Given, Current produced by alternator = 1.540 A Engine operations requires = 1.179 A  mass of…

Q: A current of 5.90 A is passed through a Sn(NO3)2 solution. How long, in hours, would this current…

A: The solution is having salt Sn(NO3)2 which contains ion Sn2+  Hence on passing the current, below…

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

A:

Q: What mass of Ba(s) may be deposited from an aqueous BaCl2 solution if a current of 2.50 A is applied…

A: Mass of electrodeposited species can be calculated from the amount of charge passed.

Q: Oxygen Supply in Submarines Nuclear submarines can stay under water nearly indefinitely because they…

A: The electrolysis of water produces oxygen. Since the O is in 2- oxidation state in water initially…

Q: How long must a current of 5.00 A be applied to a solution of Ag + to produce 10.5 g silver metal?

A: The electrolysis reaction taking place to produce Ag (s) from Ag+ (aq) solution will be  Ag+ (aq) +…

Q: (a) In the electrolysis of aqueous Na2O2, how many liters of H2(g) (at STP) are generated by a…

A: The reaction taking place is given as, => Na2O2 (aq) + H2O (l) ↔ H2 (g) + O2 (g) + NaOH (aq)…

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: Over a period of time, the concentration of sulfuric acid in the lead storage battery of an…

A: Given data,Initial % by mass of H2SO4=38.0 %Final % by mass of H2SO4=26.0%Volume of H2SO4=734…

Q: How long will it take to plate out 1.2 g Ni from aqueous Ni2+ with a current of 112.4 A? WHERE ARE…

A: Given,   1.2 g Ni plate out from aq Ni2+ with a current of 112.4 A

Q: Weighing a copper atom in an electrolysis experiment. A standard experiment involves passing a…

A: Electrolysis is the process through which electrical energy is converted into the chemical energy…

Q: A current of 0.10A has flown through a solution for 3.00 minutes. How many electrons have passed…

A: Given: 1 C = 1 A.s   Therefore, for the current of 0.1 A passed through 3.00 minutes, number of…

Q: What mass of Sn(s) may be deposited from an aqueous SnCl, solution if a current of 2.50 A is applied…

A: Given,

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 long would it take a current of 1 ampere to reduce completely 80 cm3 of 0.10 M Fe2(SO4)3 to…

A: We can solve this problem by using the faraday law of electrolysis  W= (E×i×t)/96500 W= mass of a…

Q: How many minutes are required to deposit 3.77 g Cr from a Cr³⁺(aq) solution

A: We will calculate time for deposit of metal

Q: A current of 0.500 A flows through a cell containing Cd(II) for 10.0 minutes. Calculate the maximum…

A: During electrolysis cadmium deposited as solid. The mass or moles of metal deposited can be…

Q: How long will it take to plate out 4.2 g Ni from aqueous Ni2+ with a current of 112.3 A? HOW DO WE…

A:

Q: 1) What is measured in Volts? a) how many electrons are passing through a system b) how many…

A: "To get remaining sub-parts solved please repost the complete question and mention the sub-parts to…

Q: What mass of Pb(s) may be deposited from an aqueous PbCl, solution if a current of 2.50 A is applied…

A: The correct option is:

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.