Elemental calcium is produced by the electrolysis of molten CaCl2. (a) What mass of calcium can be produced by this process if a current of 7.5 * 103 A is applied for 48 h? Assume that the electrolytic cell is 68% efficient.

Q: How many moles of oxygen, O2, will be produced by the electrolysis of water with a current of 1.5…

A:

Q: The electrolysis of T(Br3 at high temperature produces thallium metal. If a constant electrical…

A: First we have to find how much charge is required for one mol thallium. Then find how much current…

Q: What mass of aluminum will be deposited in 1.00 hours by the electrolysis of molten AlCl 3 using a…

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Q: Calculate the mass of Li formed by electrolysis of molten LiCl by a current of 7.5 * 104 A flowing…

A: the problem is related to Faraday`s 1st Law of Electrolysis, states that " mass of the substance…

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: Molten RbCl can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

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Q: An electrolytic cell contans 50.0 mL of a 0.152 M solution of FeCl3. A current of 0.775 A is passed…

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Q: If the potential of a cell is 0.51 V at 25°C when [Zn2+(aq)]=0.111M and the pressure of the hydrogen…

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Q: How many hours does it take to form 15.0 L of O, measured at 750 torr and 30°C from water by passing…

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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: The electrolysis of TℓBr3 at high temperature produces thallium metal. If a constant electrical…

A: From Faradays first law, weight of the substance deposited, W = ZQ Z = E/F = equivalent…

Q: In the commercial production of sodium metal by electrolysis, the cell operates at 7.0 V and a…

A: Given: Potential=7.0V current=25×103A Time=1h=3600s To find: The mass of metallic sodium produced in…

Q: How many moles of oxygen, O 2, will be produced by the electrolysis of water with a current of 1.5…

A:

Q: Aluminum is produced commercially by the electrolysis of Al, O3 in the presence of a molten salt. If…

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Q: Molten RbCl can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

A: we know the expression for the  faraday's law of electrolysis => m/E = It / F Where,  I is the…

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…

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A: Here we have to determine the time required to deposit 75 g of iron in the elctrosysis of FeCl3 by…

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: 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: A galvanic cell is based on the following reaction(at 25°C)： Cu (aq)+Sn(s) → Cu(s)+Sn (aq) If the…

A: Note - The given reaction is incorrect. So, we will use the correct reaction for the question.   A…

Q: How many seconds does it takes to produce 5.0 L of aluminum sulfide, Al2S3 measured at 0.95 atm and…

A: Using ideal gas equation, we have P×V = n×R×T     -----(1) Where, P is pressure             , V is…

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: 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: Question three on photo

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

Q: Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If…

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Q: Electrolysis of a solution of Zn(NO3)2 (aq) to give zinc metal is carried out using a current of…

A: The expression for the mass of metal deposited is given as:

Q: (4) When a metal of molar mass 207 g mol" is deposited by electrolysis, a current of 0.06 A flowing…

A: Convert the unit of time: 1 min=60 s66 min=66 min×60 s1 min=3960 s

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: (a) How long (in hours) does it take to produce 454 g of copper from a solution containing Cu²*…

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Q: The electrolysis of AℓCℓ3 at high temperature produces aluminium metal. If a constant electrical…

A: Given: current = 10 × 103 mA Or current = 10 × 103 × 10-3 A Or current = 10 A And time = 1 hour =…

Q: How many grams of gold can be produced when a solution of Au(OH)3 undergoes electrolysis at a…

A: Faraday's first law :-  The mass of a substance deposited at the electrode is directly proportional…

Q: A major source of sodium metal is the electrolysis of molten sodium chloride. What magnitude of…

A: The  current is required to produce 1.0 kg of sodium metal in one hour is calculated as,

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 long will it take to plate out 0.270 g of iron metal from a solution containing Fe3+(aq) in an…

A: Electrochemistry is branch of chemistry in which we deal with oxidation and reduction reaction…

Q: How many grams of metal Ca (40.08g/mol) are produced by electrolysis of CaBr2 using a current of 28…

A: Kindly get the answer given below.

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: In the electrolysis of aqueous NaCl, how many grams of Cl2 are generated by a current of 2.35…

A: moles of electrons  =6.2x1018 x2.35x140x60/6.022x1023 =20454 x 10-5 =0.2 Moles of electron = number…

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

A: According to Faraday's 1st law weight of the substance from in each electrolyte  W = ZIt where , W…

Q: An electrolytic cell produces aluminum from Al2O3 at the rate of ten kilograms a day. Assuming a…

A: The formation of Al from Al2O3 is as follows: 2Al2O3(s)→4Al(s)+3O2(g) Calculation of no. of mol of…

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: 7. How many grams of aluminum metal (26.982 g/mol) can be produced by the electrolysis of Al2O3…

A: In Al2O3, the oxidation number of Al is +3 and that of O is -2.  Hence uring electrolysis of Al2O3,…

Q: Calcium metal is obtained by direct electrolysis of molten CaCl2. If a metallurgical electrolysis…

A: Calcium metal is obtained by direct electrolysis of molten CaCl2. If a metallurgical electrolysis…

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A: A numerical problem based on electrolysis that is to be accomplished.

Q: How much silver was there in the solution if all the silver was removed as Ag metal by electrolysis…

A: Given, Time (t) = 0.60 hr = 2160 s Current (I) = 1.00 mA = 1.00 × 10-3 A Amount (in grams) of silver…

Q: A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper II)…

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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: 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: How many hours does it take to form 15.0 L of O, measured at 750 torr and 30°C from water 2 by…

A:

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.