What mass of each of the following substances can be produced in 1.4 h with a current of 10. A? (a) Co from aqueous Co2+ (b) Hf from aqueous Hf4+ (c) I2 from aqueous KI (d) Cr from molten CrO3

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: During a period of discharge of a lead–acid battery, 402 gof Pb from the anode is converted into…

A: Overall cell reaction is Pb(s) + PbO2(s) + 2H+ (aq) + 2HSO4- → 2 PbSO4 + 2H2O Where, 1 mol of Pb is…

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 long will it take for a uniform current of 6.00 A to deposit 78.0 g gold (197.0 g/mol) from a…

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Q: To what pH should you adjust a standard hydrogen electrode toachieve an electrode potential of…

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

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Q: How long would it take to electroplate all the Zn^ 2+ in 0.280 L of .210 M ZnSO 4 solution with a…

A: The question is based on the concept of electrochemistry. It involves  application of first law of…

Q: How long will it take to plate out 3.0 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

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Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: The call reaction at anode is, H2(g) ------> 2H+(aq) + 2e- Standerd cell potential of the cell =…

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: Equivalents of H+ ions reduced = QF=I×t96500=11.3 ×73 ×6096500= 0.513 Total equivalents of H+ ions…

Q: The passage of a current of 0.750 A for 25.0min deposited 0.369 g of copper from a CuSO4 solution.…

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Q: A solution of a metal ion M 3+(aq) is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19…

A: The given data contains,       current =5 A      time =10 min60s1 min=600s

Q: How many grams of cadmium are deposited from an aqueous solution of cadmium sulfate, CdSO4, when an…

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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: How long (in hours) must a current of 4.61 amps be passed to produce 79.5 g of copper metal from a…

A: Given:: Current i= 4.61 A  Mass of Cu = 79.5 g  Molar mass of Cu= 63.55 g mol-1 Time t= ?

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: A constant current of 0.712 A is passed through an electrolytic cell containing molten BaCl2 for…

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Q: How long, in hours, must a current of 5.00 A be applied to a solution of Ag+ to produce 10.5 grams…

A: From the combination of Faraday's first and second law, we have : m = ItM/Fz  Or, t = mFz/IM ...(1)…

Q: 9. A concentrated Pb(NO3)2 (aq) solution is electrolyzed using a current of 10.5 A. a) What mass of…

A: SOLUTION: Step 1: Hello. Since the question contain multiple sub-parts, the first three subparts are…

Q: 3.4 How many grams of cadmium are deposited from an aqueous solution of cadmium sulfate CdsO4 when…

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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: Brass, an alloy of copper and zinc, can be produced by si-multaneously electroplating the two metals…

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Q: Question three on photo

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

Q: 2+ A current of 3.40 A is passed through a solution containing Cu²+ (aq) for 30.0 minutes, with…

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Q: Calculate the standard Gibbs energy in kJ/mol change for the following voltaic cell A(s) | A3+(aq)…

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Q: A galvanic cell consists of a Mg electrode in 1 M Mg(NO3)2 solution and a Ag electrode in 1 M AgNO3…

A: Given- Electrodes Mg  in 1 M Mg(NO3)2 solution Ag  in 1 M AgNO3 solution Temperature = 25 °C   To…

Q: If a standard cell potential is E°cell = +0.85 V at 25 °C, is the redox reaction of thecell…

A: The standard condition for a reaction to be a spontaneous is the standard cell potential is E°cell…

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

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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: Tin-plated steel is used for "tin" cans. Suppose that in the production of sheets of tin-plated…

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Q: = +0.851Vwhat is the spontaneous reaction between these two half-cells and what is the poten

A: For Spontaneous reaction, E°cell is positive.  Electrode with higher standard reduction potential…

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: Given: Concentration cell of hydrogen. Temperature = 298 K. Concentration of H+ in cathode = 1.00 M…

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

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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: If the standard voltage of the reaction of Cu(s) with Ag*(aq) is 0.46 V, what is the standard gibbs…

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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: A steady current of 3 A is maintained for 10 mins in AgNO3 solution. How much Ag is deposited at the…

A: Given: Current is 3 A. Time is 10 minutes. To find: Mass of Ag on cathode

Q: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

Q: How many seconds are required to deposit 0.184 grams of zinc metal from a solution that contains…

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Q: What mass of each of the following duced in 1.0 h with a current of 15 A? a. Co from aqueous Co2+ b.…

A: Explained as follows

Q: A solution of CuSO4 is electrolysis for 10 minutes with a current of 1.5 amperes. What is the mass…

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Q: A pure organic acid sample (0.1516 g) is neutralized with OH- ions produced in a constant current of…

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Q: DE What mass of each of the following substances can be duced in 1.0 h with a current of 15 A? pro-…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: If a solution of CuCl2 is electrolyzed, what reaction will occur at the anode when the minimum…

A: In the electrolysis process, the cations move towards the cathode and the anions move towards the…

Q: The emf of the cell Pt | H2 (1 bar) | HCl (aq) | AgCl (s) | Ag was found to be 0.517 V at 25oC.…

A: Given cell notation is  : Pt | H2 (1 bar) | HCl (aq) | AgCl (s) | Ag  EMF of the cell = 0.517 V…

Q: The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a CuSO, solution.…

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Q: A voltaic cell is constructed with two hydrogen electrodes. Electrode 1 has PH2 = 1.00 atm and an…

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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.