Silver can be plated out of a solution containing Ag+ according to the half-reaction:Ag+(aq) + e------->Ag(s)How much time (in minutes) does it take to plate 12 g of silver using a current of 3.0 A?

Q: The answer is -1.98V

A: To calculate the standard cell potential for the given reaction and determine its spontaneity, we…

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

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Q: Consider the standard reduction potentials and redox couples used in a galvanic cell. Unbalanced…

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Q: Cr³*(aq) + 3 e¯ → Cr(s) E°red = -0.744 V Zn**(aq) + 2 e → Zn(s) E°red = -0.763 V Given that the…

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Q: How long would it take to deposit 3.75 g of iron from an aqueous solution of iron (III) sulfate by…

A: According to Faraday's First Law of Electrolysis, the chemical deposition due to flow of current…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr3+ (aq) +…

A: We can use Nerst Equation to solved the above problem.

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3 e → X(s)…

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Q: Fe(s) + 2Ag* (aq) → Fe2* (aq) + 2Ag(s) (a) What is being oxidized, and what is being reduced? (b)…

A: In galvanic cell chemical energy is converted to electrical energy through an spontaneous reaction.

Q: Write the two half-reactions of the following redox reaction. Calculates the difference between the…

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Q: ) Consider the galvanic cell, Zn(s) | Zn2+(aq) || Pb2+(aq) | Pb(s). Which one of the following…

A: Galvanic cell : The notation in galvanic cell is written as : So , the reaction for given cell…

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3 e X(s)…

A: E° cell = E° cathode + E° anode  At anode always oxidation occur  At cathode always reduction occur…

Q: How many grams of Ag would be deposited from an aqueous solution of Ag+ with a current of 2.534 A…

A: Molar mass of Ag = 108g/mol Reaction takes place:- Ag+ + e-  ------> Ag  current , I = 2.534 A…

Q: Consider these two entries from a fictional table of standard reduction potentials. X³+ + 3e → X(s)…

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Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

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Q: temperature is 38°C and the operating pressure is 0.04 atm. Cd2*(aq) + 2 e- → Cd(s); [Cd²*] = 0.50 M…

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Q: Electrolysis of an aqueous solution of sodium chloride produces chlorine, . The reaction that occurs…

A: Give that: the reaction of anode is: 2Cl- (aq) →Cl2 (g) + 2e- Mass of Cl2 produced, w =182 g, time…

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Q: A particular voltaic cell operates on the reaction Zn(s) + Cl, (9) → Zn+ (aq) + 2C1 (aq) giving a…

A: The given equation is, The anode reaction of given cell is, The cathode reaction of given cell is,…

Q: Using the reaction between Fe(NO3)2(aq) + Al(s) complete each of the following. Single displacement…

A: as you've asked a multipart question we are going to solve first three questions for you if you want…

Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: X3+ +3e- ⟶ X(s) , Eo =−1.63 V (anode) Y3+ +3e−⟶Y(s), Eo =−0.41 V (cathode)

Q: The cell potential for a voltaic cell composed of zinc and copper is 1.0 V under standard…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: This galvanic cell uses the reaction: Cu(s) + 2 Ag*(aq) → 2 Ag(s) + Cu2+(aq). f a C oxidation half…

A: Standard Reduction potential of Cu2+ = 0.34 v . Standard Reduction potential of Ag+ = 0.80 v. Ions…

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.