In the electroplating of nickel, 0.200 faraday of electrical charge is passed through a solution of NISO4. What mass of nickel is deposited? O 2.94 O 5.87 O 11.7 O 58.7

Q: A solution of nickel(II) ion (Ni2+) is electrolyzed using a current of 15.0 A (amperes) for 25.0…

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Q: Calcium metal can be obtained by the direct electrolysis of molten CaCl2, at a voltage of 3.2 volts.…

A: Given data: Given voltage = 3.2 volt Atomic weight of Calcium = 40.078 g/mol

Q: Calculate the charge, in coulombs, is required to deposit 1.5 g of solid magnesium from a solution…

A: The answer to the following question is- Given, mass of magnesium = 1.5 g  Molar mass of magnesium =…

Q: The reactions occurring at (i) anode, (ii) cathode, during working of a mercury cell. Why does the…

A: A voltaic cell is an example of electrochemical cell. It uses a chemical reaction to produce…

Q: An electrolysis cell for aluminum production operates at 5.0 V and a current of 8.5 x 10° A.…

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Q: In acidic conditions, manganate(VII) ions are reduced to manganese(II) ions, Mn. In neutral…

A: The balanced equations for the reduction of manganate(VII), MnO4-(aq) in acidic and neutral medium…

Q: Determine the mass of Sodium (Na) produced when a 373 amp current flows for 7 hr through a cell…

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Q: How much energy is consumed to produce 1.00 kg of magnesium by electrolysis of molten MgCl2 using a…

A: Given: Mass of magnesium = 1.00 kg Current                     = 1.5 x 103 A Voltage…

Q: Describe the process that releases electrons in a zinccoppervoltaic cell.

A: Given voltaic cell = Zinc-copper  Describe the process that releases electrons in a zinc-copper cell…

Q: Calculate the number of grams of aluminum produced in 1.00 h by the electrolysis of molten AlCl3 if…

A: Given: Electrical current = 10.0 A Time of electrolysis = 1.00 h.

Q: Cadmium metal can be prepared by electrolysis of its aqueous salts   A. True   B. False

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Q: In the Hall-Heroult process, a large electric current is passed through a solution of aluminum oxide…

A: The equation of deionization for aluminum is

Q: A steady current was passed through molten CoSO. until 2.35 g of metallic cobalt was produced.…

A:

Q: 22056 This substance can be stretched into a wire. a, jonic b. covalent 4. C. metallic d. none of…

A: Here we are aksed to choose the correct one in the given options .

Q: A 0.250M solution of Na2C2O4 is to be used in a reaction in which C2O-24 will be oxidized to CO2.…

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Q: Using the standard reduction potentials listed in Appendix E, calculate the equilibrium constant for…

A: The equilibrium constant K represents the relation between the reactants and products of a chemical…

Q: Which metal can be added to steel to form an alloy, which is resistant to corrosion, known as…

A: Stainless steel is the steel which is resistant towards corrosion. It contains approximately 10.5%…

Q: Write a balanced equation to represent the electrolysis of molten sodium chloride. What volume of…

A: A balanced equation to represent the electrolysis of molten sodium chloride has to be given.

Q: Using the table of standard reduction potentials, determine the net redox potential of the reaction,…

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Q: Calcium metal can be obtained by the direct electrolysis of molten , at a voltage of 3.2 volts. How…

A: Given voltage = 3.2 V Atomic weight of Calcium = 40.078 g/mol

Q: Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction…

A: Given data, ∆H° = 180.50 KJ = 180500 J ∆S° = 24.77 J/K Temperature (T) = 25°C = (273+25) = 298 K

Q: 8. Which of the following is NOT produced during the electrolysis of water? Electricity a) b) Acid…

A: we have to select the option which is  not produced in electrolysis of water

Q: How many grams of Ca metal are produced by the electrolysis of molten CaBr2 using a current of 30.0…

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Q: How many grams of Ca metal are produced by the electrolysis of molten CaBr2 using a current of 30.0…

A: Given,  Current (I) = 30.0 amp Time (t) = 8.0 hours = 8.0 × 60 × 60 sec = 28800 sec Mass (in grams)…

Q: An electrolysis cell for aluminum production operates at 4.0 V and a current of 8.5 x 10° A.…

A: The solution is given below -

Q: In the Hall-Heroult process, a large electric current is passed through a solution of aluminum oxide…

A:

Q: Calculate the potential for the electrochemical cell made from zinc and magnesium and their…

A: To find electrode potential.

Q: Calculate the mass of aluminum produced in 1.00 hour by the electrolysis of molten AlCl3 if the…

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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: Electrolysis plays an important role in the manufacture or purification of all of the following…

A: There are different type of compounds, which are synthesized by different methods -  (1) Sodium, Na…

Q: Gold (atomic mass = 197.0) is plated from a solution of chloroauric acid, HAuCl4; it deposits on the…

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Q: In the Hall-Heroult process, a large electric current is passed through a solution of aluminum oxide…

A: Amount of pure aluminium formed can be calculated from the moles of charge passed.

Q: one of the following metals is used as oxidizing agent a. Ca b. Na c. Fe+2 d. Fe+3

A: Oxidising agent :- The oxidizing agents are those species which can oxidise other species and can…

Q: Calcium metal can be obtained by the direct electrolysis of molten Cacl2, at a voltage of 3.2 volts.…

A: Given: Voltage = 3.2 V And mass of Ca required = 5.28 Kg = 5280 g…

Q: Which element is oxidized in the reaction?   Fe2O3 + Al →Al2O3 + Fe

A: Which element is oxidized in the reaction? Fe2O3 + Al →Al2O3 + Fe

Q: Aluminum is produced commercially by the electrolysis of Al203 in the presence of a molten salt. If…

A: Total current, I = 1.09 million Ampere                           = 1.09×106 Ampere Time, t = 3 hr…

Q: In the Hall-Heroult process, a large electric current is passed through a solution of aluminum oxide…

A: we will apply the combined Faraday's law W = (Q*M )/F*n  W = weight of mass in grams Q = quantity of…

Q: What mass of chromium could be deposited from a solution of Cr3+ (aq) using a current of 10.0 A for…

A: Q = IT = 10 A * 10800 sec = 108000 C Q / F = 108000 / 96500 = 1.119 mole e- This is a 3 electron…

Q: How many grams of silver are deposited at a platinum cathode in the electrolysis of AgNO 3 (aq) by…

A: Given: Current, I = 5.30A Time, t= 4.0hr = 4 x 60x 60 s = 14400s And we know, Equivalence mass of…

Q: Write a balanced half-reaction describing the oxidation of solid magnesium to aqueous magnesium…

A: Given: Oxidation of magnesium to magnesium cation.

Q: Calculate the mass of chlorine in grams that can be produced by the electrolysis of 50.0 kg of…

A: The electrolysis of sodium chloride takes place as follows: 2NaCl(aq) + 2H2O(l) → 2NaOH(aq)+ Cl2(g)+…

Q: A metal forms the fluoride MF3. Electrolysis of the molten fluoride by a current of 3.86 A for 16.2…

A: The current produced, I = 3.86 ATime, t = 16.2 min = 972 sMass of metal deposited, m = 1.25 g

Q: An electrolysis cell for aluminum production operates at 4.5 V and a current of 7.5 x 10° A.…

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Q: How many minutes will it take to plate out 4.56 g of Ni metal from a solution of Ni2+ using a…

A: Given: Mass of Ni deposited = 4.56 g Current passed = 45.5 A Molar mass of Ni = 58.69 g/mol

Q: Aluminum metal is produced by electrolysis of Al½O; in molten cryolite (Na3AlF6). (a) If the…

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Q: What volume of Oxygen at STP can be produced by the electrolysis of 20.0 g water?…

A: Balanced chemical equation for electrolysis of water is given by 2 H2O (l) → 2 H2 (g) + O2 (g) Mass…

Q: What are the products obtained by the electrolysis of a solution of aluminum chloride? Cl2(g),…

A: Electrolysis in a process defined by in which dissociation of electrolytes happen by the passage of…

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: Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved…

A: ∆G= +150KJ/mol = 150×103J/mol F= 9.649 x 104C For group element, n= 2

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.