A voltaic cell consists of a silver electrode in contact with 325 mL of 0.100 M AgNO3 solution and a magnesium electrode in contact with 275 mL of 0.100 M Mg(NO3)2 solution.  The battery operates at 25°C drawing electrons from the magnesium electrode to the silver electrode. Calculate the voltage of the voltaic cell (Ecell) after 0.50 grams of silver have been deposited on the initial surface of the silver electrode.

Q: A voltaic cell is constructed with two Zn2+−ZnZn2+−Zn electrodes. The two cell compartments have…

A: The cell is made up of Zn electrodes only. Hence both oxidation and reduction is happening for Zn…

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

A:

Q: Three electrochemical cells were connected in series so that the same quantity of electrical current…

A: Concept introduction: Faradays second law of electrolysis is explained as when the same quantity of…

Q: This galvanic cell uses the reaction: Zn(s) + 2 Ag*(aq) 2 Ag(s) + Zn2+(aq) The initial…

A: The cell reaction given is, => Zn (s) + 2 Ag+ (aq) -------> 2 Ag (s) + Zn2+ (aq) Given :…

Q: n electrochemical cell is constructed in which both electrodes are pure iron immersed in a solution…

A: Solution - The correct option is (A)

Q: A voltaic electrochemical cell is constructed using the following reaction. The half-cell components…

A: The reactions at cation and anion are given below.

Q: what is the combination of electrodes that would generate the greatest voltage in a galvanic cell?

A: Answer: The greatest voltage occurs when the difference in the reactivity of the two metals is the…

Q: What is the maximum amount of electrical work that can be done when 50.5 grams of PbO2 is converted…

A: The rxn for the lead acid battery is given as   and we have to calculate the energy in terms of kJ…

Q: How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous…

A: The balanced chemical equation for the reduction of copper is: Thus, for the production of 1 mole…

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 student does an experiment to determine the molar solubility of lead(II) iodide. She constructs a…

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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: Under standard conditions, the ΔGo of the reactants for a given redox reaction is measured to be…

A: Since the relationship between the Eocell and the ΔGo is given by  ΔGocell = -nFEocell  where n =…

Q: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

A: We will calculate the standard reduction potential at 25 degree centigrade.

Q: A laboratory was assigned the job of determining the copper(II) ion concentration in thousands of…

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Q: A certain metal M forms a soluble sulfate salt MSO 4. Suppose the left half cell of a galvanic cell…

A: We are dealing with a concentration cell where both half-cells contain the same metal ions but at…

Q: An electrochemical cell is set up with the following configuration: Hg|Hg2+||Mn2+|Mn.  The solutions…

A: Spontaneity of a Chemical reaction in a galvanic cell on the basis of cell potential:

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: Use the attached picture to help answer the question. The image shows a galvanic cell with Ag as…

A: To answer the question : The image shows a galvanic cell with Ag as one electrode and Sn as the…

Q: Consider the following working voltaic cell with a positive voltage: Cu(s) | Cu²+ (aq) || Ag* (aq)|…

A: Redox reactions are reactions in which both oxidation and reduction takes place together. In a…

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

A: Given data,Current=29.0ATime=69.0sReaction at cathode;Pb2++2e-→Pb(s)

Q: Calculate the Ecell for a voltaic cell made of a strip of metallic Ga dipped into 0.311 M…

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

A:

Q: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

A: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

Q: If the standard potential of a voltaic cell is + 0.831 V, what is the standard free-energy change…

A: Given standard cell potential of the Voltaic cell, Eocell = 0.831 V  Given the number of electrons…

Q: Consider the galvanic cell. In a certain experiment, the emf () of the cell is found to be Q.54 V at…

A: Solution :    Nernst equation is used to calculate the potential of the cell at non-standard…

Q: A certain metal M forms a soluble sulfate salt MSO 4. Suppose the left half cell of a galvanic cell…

A: Which electrode will be positive?The right electrode will be positive.This is because the…

Q: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that  An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

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

A:

Q: Consider the voltaic Cell shown below. Voltaic Cell V Voltmeter Salt Ag (s)-> bridge Cd (s) Ag+ (aq)…

A: 1) 2.82 V2) Ag3) CdExplanation:

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

A:

Q: Find the voltage of the cell if the right half-cell contains 0.330 M AgNO₃ (aq) and the left…

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

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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.