What is the electrical current, in Amperes, that must be applied if 6.50 g Ag is deposited at the cathode in 2.00 hrs during the electrolysis of AgNO3 (aq)?

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

A: The reaction given is, Cu2+aq+Zns→Cus+Zn2+aq Cu2+ is being reduced to Cu and Zn is being oxidised to…

Q: Balance the following reaction. Calculate the cell potential and the Gibbs free energy of the…

A: The questions are based on the concept of redox reactions.   Redox Reaction  are those reactions in…

Q: In the electrolysis of water, how long will it take to produce 155.0Lof H2 at 1.0 atm and 273 K…

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

A: The given reaction is, 2Cr3+aq+3Cas→2Crs+3Ca2+aq The half cell reactions and their standard…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210,…

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

A: In cell notation anode is written on left side and cathode on right side.

Q: (a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a…

A: i = 81.2 A t = 59.2 min

Q: Calculate the cell potential for the galvanic cell in which the reaction   Fe(s)+Au3+(aq)↽−−⇀…

A: Please find your solution below :

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: 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: How much Ca will be produced in an electrolytic cell of molten CaCl2 if a current of 0.452 A is…

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Q: Manganese dioxide (MnO2) for use in dry cell batteries is made by electrolyzing solutions of Mn2*…

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Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 210, (aq)+…

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Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3 Cu²+ (aq)…

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Q: Given the reaction    4 Al(s) + 3O2(g) ===>  2Al2O3(s), write the half reactions and calculate…

A: The reaction given is, => 4 Al (s) + 3 O2 (g) --------> 2 Al2O3 (s)

Q: Write the cell notation for an electrochemical cell consisting of an anode where H2 (g) is oxidized…

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Q: Copper is plated onto the cathode of an electrolytic cell containing CuCl2(aq). How long does it…

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Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3 Cu²+…

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

A: In this question, we will write cell notation for given anode and cathode half cell Reaction. How we…

Q: Write the cell notation for an electrochemical cell consisting of an anode where H2 (g) is oxidized…

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Q: What mass of zinc (in grams) is deposited at the cathode when a current of 8.3 amperes passes…

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

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Q: The following cell Ag | Ag+(0.10M) || Ag+(1.0M) | Ag is a concentration cell and is capable of…

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Q: In a galvanic cell, a full redox reaction takes place, one half-reaction at each electrode. How is…

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Q: When building a galvanic cell, what is the importance of the molecule in the anode vs the cathode.…

A: Galvanic cell converts chemical energy into electrical energy. Here Zn rod is dipped in ZnSO4…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr2+ (aq) is…

A: In the standard cell notation, the single vertical line represents the phase boundary and the double…

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

A: The cell reaction taking place is given as, => Sn2+ (aq) + Ba (s) -------> Sn (s) + Ba2+ (aq)…

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

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Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 210, (aq) +…

A: Oxidation is lose of electrons. Reduction is gaining of electrons. Galvanic cell is an…

Q: Enter your answer in the provided box. The MnO, used in alkaline batteries can be produced by an…

A: Please find the answer attached here as handwritten note.

Q: ulate the potential of the following cells: a galvanic cell consisting of a lead electrode on the…

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Q: How long ( hours) would it take to unload 0.433 moles of vibranium (Vb) metal during electrolysis of…

A: We have to calculate time needed for electrolysis  Molar mass of Tr not provided so only 1st…

Q: Oxygen Supply in Submarines Nuclear submarines can stay under water nearly indefinitely because they…

A: The electrolysis of water produces oxygen. Since the O is in 2- oxidation state in water initially…

Q: Suppose somebody in the laboratory doesn’t quite turn off the current in an electrolysis cell so…

A: The relation between charge and time is shown below: Q = It where; Q = charge I = current t = time

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

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Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn²+…

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Q: For the galvanic cell  2Ag+ + Cr  →  2Ag + Cr2+,  which equation allows you to correctly calculate…

A: E°cell = 2.5122 V

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 2.1…

A: We have given that during the electrolysis of molten Sodium chloride 2.1 g of Sodium is produced at…

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

A: The reaction given is Hence in the above reaction, Cr3+ is being reduced to Cr and Ca is being…

Q: Consider the following electrochemical cell notation with a cell potential of 0.300 V. Pt ∣Cr3+(aq,…

A: NOTE : There is a minor correction in the cell notation given. As per the rules, the specie which is…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Sn²* (ag)+Ba…

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Q: A constant current is passed through an electrolytic cell containing molten MgCl2 for 18 h. If 4.33…

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

A: The reaction given is Hence in the above reaction, Cu2+ is being reduced to Cu and Zn is being…

Q: products

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Q: a galvanic cell is constructed from a standard hydrogen electrode and from another hydrogen…

A: A numerical problem about galvanic cell constructed using two Hydrogen electrodes.

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu2* (aq)+…

A: The cell reaction taking place is given as, => 3 Cu2+ (aq) + 2 Al (s) -------> 3 Cu (s) + 2…

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

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Q: Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction…

A: The balanced redox reaction can be written as: MnO4- + 8H+ + 5e-  →  Mn2+ + 4H2O (Reduction)5Ce3+  →…

Q: How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current…

A: Faraday's law of electrolysisAsW= Ite/FF= 965900 Ct=20 x 60 sece for copper if taken in copper…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu*…

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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.