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

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

A: Faraday’s first law of electrolysis:                 The mass of the substance deposited at the…

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: 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 amperes of current needs to be passed through molten Sodium chloride to produce 2.4 g of…

A: Faraday's First law,           m α Q          m = eQ               = ect               = E96500ct…

Q: How many seconds will be required to produce 1.00 g of nickel metal (58.693 g/mol) by the…

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Q: It took 116 hours to produce 603 g of metal X by performing electrolysis on molten XC13 with a…

A: From Faraday’s first law of electrolysis the quantity of charge is calculated as: Where, Q is…

Q: se a current of 770. mA flows through a copper wire for 10.0 minutes. Calculate how many moles of…

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Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 4.65…

A: Question is based on first law Faraday's law of electrolytes. i.e., amount of substance deposited is…

Q: How many grams of Au would be deposited from an aqueous solution of Au 3+ with a current of 2.213 A…

A: Given, Molecular mass of Au = 196.96 u Current = 2.213 A time = 480 minutes = 28,800 sec

Q: 3. A factory wants to produce 1.0 x 103 kg Barium from the electrolysis of molten barium chloride.…

A: The given values are: m=1.0×103 kg=1.0×106 gt=4.0 h=4.0 ×3600 s The electrolysis step to form barium…

Q: How many seconds are required to produce 8.00g of aluminum metal from the electrolysis of molten…

A: Assume that the required seconds as x. 1 A = 1 C/s. Coulombs generated by 12.0 A in x seconds is 12…

Q: What mass of copper , in mg , can be deposited from copper (II) sulfate solution using a current of…

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Q: 7. Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: If a water electrolysis cell operates at a current of 7.8 A, how longwill it take to generate 25.0 L…

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Q: Aluminum metal can be made from aluminum ions by electrolysis. What is the half-reaction at the…

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Q: What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for 143…

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Q: state and explain Faraday’s laws of electrolysis. What is Electrochemicalequivalent?

A: Faraday’s first law of electrolysis states that the mass of the substance accumulated or released at…

Q: Calculate the amounts of Cu and Br: produced at the inert elecuvues by passing a current of 4.5 A…

A: Given: Current = 4.5 A The atomic weight of Cu =63.55 gThe atomic weight of Br2=159.8 gCharge of 1…

Q: How many minutes will it take to electroplate 42.1 g of gold by running 5.00 A of current through a…

A: In an electrolytic cell for the electrolysis of a metal conversion of electrical energy in to…

Q: Electrolysis of water at room temperature yielded oxygen gas at platinum anode by using current of…

A: On electrolysis of water oxygen gas is evolved at anode. From 96500 C of electric charge moles of…

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: 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: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 3.10…

A: Formation of Cl2 from NaCl is shown below,

Q: How long will it take to plate 2.5 g of copper onto a light fixture using a solution of Cu(NO3)2 and…

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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: What volume of chlorine gas at standard temperature and pressure is evolved when a solution of MgCl2…

A: Provided time=1hour Molar mass of Cl2=70.906g/mol Let w gram Cl2 evolve So provided time…

Q: Calculate the mass of Li formed by electrolysis of molten LiCl by a current 6525 A flowing for a…

A: Given, Current = 6525 A or 6525 C/sTime = 50h = 50×3600 s = 180000seconds

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: Given: Current (I) = 11.3 A     Volume of solution (L) = 1.25 L    Concentration of HBr = 0.552 M…

Q: Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature and…

A: It is given that MgCl2 is electrolysed and a current of 12.4 A is passed for 1h.

Q: 4.) What mass of silver can be plated onto an object in 45 minutes at 9.0 A of current?

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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 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 grams of chlorine can be produced by the electrolysis of mattersNaCl with a current of 1.02…

A: Given, Current 'i' = 1.02 A time 't' = 15 min

Q: Which products are obtained in the electrolysis of molten NaI?

A: Na metal produced at cathode and I2 produced at anode.

Q: Assume molten ACI3 is electrolyzed with a current of 15.2 A. A3+ (aq) + 3 e¯ --> A (s) Eº = 1.04 V…

A: Faraday's law of electrolysis is given by Michael Faraday. Faraday's first law depicts that the…

Q: How many grams of silver will be deposited by a current of 5.00A flowing through a cell for 10.0…

A:

Q: Suppose that a machine part requires 400 mg of copper to provide a coating that is thick enough for…

A: Given data,Current=0.5ATime=10min=10×60s=600s

Q: How many seconds

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Q: During electrorefining of Cu from CUSO4, how much time (in hours) is needed to produce 250 g Cu on…

A: When a charge Q passes through a circuit the current through that circuit can be calculated by the…

Q: What mass of silver would plate onto the cathode if a current of 7.9 A flowed through the cell for…

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Q: 19. (a) Write a balanced equation for the reaction that occurs in a car battery when the ignition…

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

A: Faraday's first law of electrolysis It states that the mass of a substance deposited on any…

Q: According to the calculation, the electrolysis formed 0.107 mol M. During this time, 7.00 g M are…

A: Given: No. of mole of  (M ) = 0.107 mole Mass of ( M ) = 7 g   Find Molar mass of ( M )= ???

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 2.30…

A: In the electrolysis process, the grams of Chlorine gas generated is calculated using,

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

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

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: A current of 5.26 A is passed through a 2Sn(NO3)2 solution. How long, in hours, would this current…

A: In Sn(NO3)2 we have Sn in Sn2+ form  Hence to get tin that is Sn from Sn2+ the reaction will be Sn2+…

Q: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 3.75…

A: In the electrolysis process, the grams of Chlorine gas generated is calculated using,

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.