How many hours does it take to form 15.0 L of O, measured at 750 torr and 30°C from water 2 by passing 3.55 A of current through an electrolytic cell?

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Q: Magnesium metal can be produced industrially by electrolysis of MgCl2. What mass of magnesium metal,…

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A: Current (I) = 4.21 A  Mass of nickel deposited (m) = 4.50 g

Q: hours will it take to plate

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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: Use the standard free energies of formation in Appendix B to calculate the standard cell potential…

A: As per the standard table standard free energy of formation is :  ∆G°f (H2) = 0 KJ/mol  ∆G°f (O2) =…

Q: (b) A constant current was passed through a solution of AuCl; between gold (Au) electrodes. After a…

A: Given, Mass of gold deposited = 2.628g Time = 20min = 1200 second

Q: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

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Q: For a hydrogen/oxygen fuel cell, with an overall fourelectron cell reaction        2 H2(g) + O2(g) →…

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Q: =

A: Given: Sn | Sn2+ (aq) =−0.140 V Pb | Pb2+(aq) =−0.126 V, T= 298 K

Q: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

A: According to Faraday's Law: W=ZIt                         ...... (1) where w is the mass formed, I…

Q: In the electrolysis of a 200 mL metal experiment, 0.0434 grams of cathode is applied when a current…

A: Given: weight of metal(w) = 0.0434  Current(I) = 0.50 A  Time(t) = 5 min = 300 sec  Valency factor =…

Q: In the electrolysis of water, how long will it take to produce 1.000 × 102 L of H2 at STP (273 K and…

A: Welcome to bartleby!  Introduction :  We have to calculate time required for electrolysis of…

Q: rent of 1.88 x 10° ampere is passed thro olytic cell for 24 hours. Calculate the m s9% efficient 80%

A: Charge = current × time Q = I × t Mass = M × Q / n × F M is the molar mass n is the number of…

Q: For the cell, H2(1 atm)|HBr(α=1)||AgBr|Ag, E is given as E = 0.07121 – 4.99 x 10-4 T – 3.45 x 10-6 T…

A: Given: E = 0.07121 – 4.99 x 10-4 T – 3.45 x 10-6 T2 T = 25 °C + 273 = 298 K

Q: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

A: In electrolysis cation is attracted towards cathode and anion is attracted towards to the anode.

Q: Devise a cell in which the following is the reaction and calculate the standard cell potential: 2…

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Q: Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

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

A: Current (I) = 84 ATime (t) = 1 hour = 3600 s mass of Zinc metal produced = ?Note:Molar mass of Zinc…

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Q: Fe (s) + O2(g) + 2H2O (l) → Fe3+ + 4OH- Balance the  simple redox reaction, If the standard change…

A: Oxidation is the loss of electrons and reduction is the gain of electrons.

Q: Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized…

A: Mg(s)|mg+2(aq,1mol/l,1atm)||cr+3(aq)|cr+2(aq,1mol/l,1atm) That is cell notation  Single line…

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Q: (a) Liquid H2O is subjected to electrolysis. One of the half-reactions is 2 H2O → O2 (g) + 4 H+(aq)…

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Q: An aqueous solution of an unknown salt of molybdenum is electrolyzed by a current of 2.50 A passing…

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Q: Molten CaCl₂ can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A: For CaCl2 , the given data is- Current(I) = 2.06A Mass of Ca = 29.3g Atomic mass of Ca = 40.078 g…

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…

A: For this problem we can incorporate Faraday's Laws of Electrolysis with the Ideal Gas Law to have…

Q: In the electrolysis of water, how long will it take to produce 1.000 × 102 L of H2 at STP (273 K and…

A: Volume of H2 produced = 100 L at STP i.e P = 1 bar = 0.987 atm and T = 273 K.

Q: Consider an electrochemical cell operating under standard conditions and at 25 °C. One half cell is…

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

A: Given:  Current (I) = 10 x 103 Amp  Time(t) = 1 hour = 3600 sec

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized…

A: In an electrochemical cell, oxidation occurs at the anode and reduction occurs at the cathode. In…

Q: A constant current is passed through an electrolytic cell containing molten MgCl2 for 13.0 h. If…

A: Given,Mass of Cl2 = 5.80 x 105 gTime = 13.0 h

Q: Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized…

A: Given,  In the cell at anode Zn(s) is oxidized to Zn2+(aq) and at cathode H+(aq) is reduced to H2(g)…

Q: * :For Electrode Potentials The potential difference between the electrodes of the cell cannot be…

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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: A student designs an ammeter (a device that measures electrical current) that is based on the…

A: The magnitude of the current in amperes is to be calculated from the given data. Given: Volume of…

Q: liters of Cl₂(g) is generated by this electrolysis. (b) How many moles of NaOH(aq) are formed in the…

A:

Q: Molten CaCl, can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A: Given-> Current (I) = 2.99 ampere Weight of Ca= 23.5 gm

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.