A galvanic cell is prepared using aluminum and nickel follows the cell notation Al(s) | AI3+(aq) || Ni2*(aq) | Ni(s). Which of the following is the correct balane spontaneous redox reaction? 3NI2*(aq) + 2Al(s) 2A13*(aq) + 3Ni(s) none of the choices Ni(s) + Al3+ (aq) Ni2*(aq) + Al(s) Ni2*(aq) + Al(s) A3+ (aq) + Ni(s) O 3Ni(s) + 2AI3+(aq) → 3NI2*(aq) + 2Al(s)

Q: Consider the following net cell reaction: 2Cu²+ (aq) + Mg (s) →→→2Cu+ (aq) + Mg²+ (aq) Which of the…

A: The question is based on the concept of electrochemistry. we need to identify correct cell…

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

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Q: A galvanic cell is constructed that carries out the reaction 2 Ag(s) + Cl2(g) -> 2 Ag+(aq) + 2 Cl2-…

A: Nernst equation is used to  calculate cell potential or  cell voltage as follows

Q: Write a balanced equation from each cell notation

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Q: A galvanic cell is prepared using aluminum and nickel follows the cell notation Al(s) | AI3+(aq) ||…

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Q: 1,Find the standard change in free energy and the equilibrium constant for the galvanic cell…

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Q: What is K for the reaction Zn(s) + Cu²*(aq) ® Zn²*(aq) + Cu(s), given E°cell is 1.1 V at 25 °C for…

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Q: Identify the anode half reaction and the cathode half reaction in the following galvanic cell: Pt |…

A: Galvanic cell :-  A device which is used to convert the chemical energy of a spontaneous redox…

Q: The following electrochemical cell is constructed at standard state: Mg(s) | Mg2+ || Cr2+ | Cr(s) a)…

A: Answers are explained below.

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq)…

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Q: In the following electrochemical cell, what is the cathode half reaction? Mn(s) | Mn2+(aq) ||…

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Q: Calculate the time (in hours) that it takes for 4.97 grams of Cr (s) to be produced when 1.647…

A: mass of Cr(s) = 4.97 gCurrent (I) = 1.647 ATime (t) = ? hourNote: molar mass of Cr = 51.9961 g/mol

Q: ELECTROCHEMISTRY (UNIT 4) Given the following reaction: Mg(s) + Zn2"(aq)→Mg²+ (aq) + Zn(s) The…

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Q: Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.30 M), Cr³+ (2.0 M) || Co²+ (0.17 M) | Co…

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Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

A: The galvanic cell contains two half-cells: Ni/Ni2+ and Co/Co2+.  Initial concentrations:  [Ni2+] =…

Q: Under standard conditions, the cell potential for a voltaic cell composed of zinc and copper is 1.10…

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Q: galvanic cell formed from the following two half-reactions? Assume that the cell temperature is 38°C…

A: Galvanic cell reaction,  Cd2+(aq) +Mg(s) --->Cd(s) + Mg2+(aq) E°cell = E°c - E°a = -0.403…

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

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Q: What would be the cell reaction and standard cell potential of a galvanic cell employing the…

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Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

A: Given-> E°Ni2+/Ni = -0.25 V E°Co2+/Co = -0.28 V

Q: 20. A galvanic cell is constructed at 25°C as indicated in the shorthand cell notation: Determine…

A: In a given question, we have to find out the free energy of Cell , equilibrium constant and cell…

Q: (b) Fe(s) | Fe²*(aq) || Ce³+ (aq), Ce**(aq) | Pt

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Q: Sketch the galvanic cell based on the following overall reactions. Calculate e°; show the direction…

A: The standard reduction potentials of the two half-cells are: Cl2/2Cl-: 1.36 VCr2O72-/Cr3+:1.33 V

Q: Calculate the [Ni2+] in the following galvanic cell, given that the measured voltage of the cell is…

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Q: According to the following cell notation, which species is undergoing oxidation? Fe(s) | Fe2*(aq) ||…

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Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

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Q: A chemist designs a galvanic cell from the following two half-reactions NO3(aq) + 4H+ (aq) + 3e →…

A: Given that, for a galvanic cell, two half-cell reactions are NO3-aq + 4H+aq + 3e- → NOg + 2H2Ol…

Q: In the given electrochemical cell, what is the cathode half-reaction? Zn(s) | Zn2+(aq) || Fe3+(aq),…

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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.