Suppose somebody in the laboratory doesn’t quite turn off the current in an electrolysis cell so that 4.2 mA of current continues to flow. If the cell then is left untouched for exactly three weeks, How many moles of electrons have flowed through the cell in that time?

Q: 7. A current of 1000. A flows for exactly 1 hour, through a cell in which the following reaction…

A: Electric current : It is defined as the rate at which a particular charge flows. It is represented…

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

A: At cathode reduction takes place while at anode oxidation takes place.  Current (I) = 1.55 A  Time…

Q: 3. A current of 0.46 A was passed through a copper (II) sulfate solution using copper electrodes for…

A: According to faraday law of electrolysis:- W=Mm*It/n*f Where W= mass lebarated of metal Mm= molar…

Q: Consider the following galvanic cell:     E° (V) U3+  +  3 e−   →   U(s) −1.642 In3+  +  2e−…

A: KCl is present in Salt bridge. Salt bridge : A salt bridge is U shaped device that connects the…

Q: A galvanic cell with a voltage of 1.3 V utilises the reaction: Zn + Cu2+ →→ Cu + Zn2+, as a source…

A: Given: The cell voltage is 1.3 V. The amount of Cu and Zn used is 6.3 g and 11 g, respectively.

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: Calculate the free energy, ΔG°, (kJ/mol) for the galvanic cell performing the following reaction as…

A: The cell reaction given is V + Sr2+ → Sr + V2+ Temperature, T = 25 °C = (25 + 273.15) K = 298.15 K…

Q: The equation for the electrolysis of a molten zinc bromide salt, ZnBr2, is shown below.  ZnBr2 (l)…

A:

Q: an irregularly shaped metal part was made from a particular alloy was galvanized with zinc using a…

A: Given The amount of current (I) is 2.15 A The time is 2.2 hours The density of zinc is 7.410 g/cm3…

Q: Consider the following galvanic cell. (Hint: Write the balanced reaction.) Cr(s)|Cr3*(aq, 1.0 M) ||…

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Q: When lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: Sketch and label a galvanic cell that makes use of the following spontaneous redox reaction. Mg(s) +…

A: A galvanic cell is an electrochemical cell that converts chemical energy to electrical energy, using…

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: Which of the following are standard conditions for an electrochemical cell?   1. Solutes in aqueous…

A: For both half cell the standard conditions are 1 M concentration when the reactants and products are…

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

A:

Q: 12. Which of the following terms can be used to describe an electrochemical cell in which a…

A: 12) Answer :- Option 2 is correct. A galvanic cell (Energy released by spontaneous redox reaction is…

Q: 42) A positive number for maximum useful work in a spontaneous process (voltaic cell) indicates that…

A: The first statement is correct. In a spontaneous process such as a voltaic cell, a positive number…

Q: 4. A galvanic cell consisting of a magnesium electrode and a standard hydrogen electrode is…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Cu2+ (aq)…

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Q: How is the amount of current flowing through an electrolytic cell related to the amount of product…

A: An electrolyte solution is a solution that generally contains ions, atoms or molecules that have…

Q: What is the maximum voltage that can be produced by a galvanic cell with the following electrodes?…

A: The objective of the question is to calculate the maximum voltage that can be produced by a galvanic…

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A: According to the Faraday's law of electrolysis, the mass of Substance liberated or deposited at any…

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.