3. A proposed battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a battery to operate for 10 hours and deliver 1.5A current, what is the minimum mass of zinc that the anode must have?

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

A:

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

A:

Q: An aqueous solution of gold nitrate is electrolyzed with a current of 0.555 ampere until 1.32 g of…

A: The relationship between charge (q), time (t), and current (I) can be given as: q=I×t…

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A: The charge carried by 610A of current in 77 seconds is the product of current and time.q is the…

Q: Consider an electrolytic cell where silver metal is plated (reduced) from an  aqueous silver nitrate…

A:

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: A 215-mL sample of a 0.500 M NaCl solution with an initial pH of 7.00 is subjected to electrolysis.…

A: Gien: Volume of a sample = 215 mL NaCl = 0.500M pH = 7 After 15 minutes, Volume removed = 10 mL HCl…

Q: In an electrolytic cell, two inert carbon electrodes were immersed in an aqueous solution of tin…

A:

Q: A proposed battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a…

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

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A:

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

A:

Q: Nickel can be produced when a current is passed through an aqueous solution of nickel (II) acetate.…

A:

Q: If a current is flowing from a battery that's used to electroplate an object with silver, how do I…

A: Given:1.45 A.hr = 1.45 amp current per hour.

Q: A solution containing vanadium (chemical symbol V) in an unknown oxcidation state was electrolyzed…

A:

Q: An alternator recharges an automobile battery when the engine is running. If the alternator produces…

A: Given, Current produced by alternator = 1.540 A Engine operations requires = 1.179 A  mass of…

Q: A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your…

A:

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A:

Q: A current of 0.46 A was passed through a copper (II) sulfate solution using copper electrodes for 16…

A: According to faraday law of Electrolysis:

Q: An electrochemical cell is constructed by dipping a zinc rod in a solution of Zn(NO3)2(aq), dipping…

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: The charge carried by one electron is 96500 C. The electrode reaction: Given that current passed is…

Q: A copper rod was purified using an electrolysis method consisting of a 1.0 M solution of copper (II)…

A: The correct answer is given below ?

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A: Current I = 1.46 A  time t = 23.1 minutes = 23.1 * 60 s = 1386 s Mass of vanadium deposited = 0.534…

Q: Electrolytic process of determining molar mass.  An electrolysis cell contains X3+ ions. When a 5.45…

A: Given: Current=5.45A Time=2.16×103s Mass of the element=8.50 g To find: Molar mass of X

Q: Electrolytic process of determining molar mass.  An electrolysis cell contains X3+ ions. When a 5.45…

A: Molar mass is defined as the mass of 1 mole of substance. Its units are g/mol. In order to determine…

Q: An aqueous solution of NaCl was electrolyzed with a current of 2.50 amps for 15.0 minutes. What…

A:

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A: When 96500 coulombs are passed through a solution of NaCl, one mole of chlorine is deposited.

Q: A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your…

A:

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

A:

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A:

Q: A galvanic (voltaic) cell contains a copper cathode immersed in a copper(II) chloride solution and a…

A: In this question, we have to find out the correct answer of given problem by the help of the…

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

Q: A quantity of electricity equal to 9.263 × 104 C passes through a galvanic cell that has an Ni(s)…

A: Given data Electricity passed=9.263x104 C Standard value of the Faraday constant is 96500 C/mole…

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.