A Ni Ni 2+Ag Ag + galvanic cell is constructed in which the standard cell potential is 1.03 V. Calculate the free energy change at 25°C when 1.00 g of silver plates out, if all concentrations remain at their standard value of 1 Mthroughout the process. What is the maximum electrical work done by the cell on its surroundings during this experiment?

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A: To calculate Standard potential , we use formula : E°cell =  E°r ( cathode ) - E°r (anode )

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Q: Use the standard free energies of formation in Appendix B to calculate the standard cell potential…

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Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

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A:

Q: Consider the following galvanic cell: Ag(s) | Ag*(3.0 × 10“M) || Fe³*(1.1 × 10³ M), Fe²"(0.040 M) |…

A: Given,

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A: Use Nerenst  equation and standard  data E (cathode) =0.53 V E (Anode) =- 0.15 V

Q: The free energy change for the following reaction at 25 °C, when [H+] = 1.15 M and [Co²+] = 0.00897…

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

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Q: What is the cell potential (E0) for a galvanic cell formed from the following two half-reactions?…

A:

Q: Cr3+(aq)  +  3e- = Cr(s)                          -0.763 V Au+(aq)  +  e-  = Au(s)…

A: GIVEN:- Cr3+(aq)  +  3e- = Cr(s)                          -0.763 V Au+(aq)  +  e-  = Au(s)…

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

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Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A:

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A: In the given question->[Sn2+] = 0.0670 M[Co3+] = 0.0365 M[Sn4+] = 0.00661 M [Co2+] = 0.00991MThe…

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Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that (Zn+) = 0.773 M and…

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Q: (E°cell

A:

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Q: Calculate the maximum work available (in kJ) from 52.3 g of aluminum in the following cell when the…

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Q: Determine the sign of the electrodes in the cell. The left side half-cell is the and charged. The…

A: Answer: The left side of the half cell is the anode and negative charge.

Q: Sketch the galvanic cell in standard conditions consisting of two half-elements IO3-, H + | I2 (E °…

A: In the galvanic cell, the standard conditions consisting of two half-elements given are: IO3-, H + |…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg² +] = 0.755 M…

A: Given,

Q: Consider the following reaction and its AG at 25.00 °C. 2 Ag+ (aq) + Cu(s) 2 Ag(s) + Cu²+(aq)…

A:

Q: The redox reaction is 2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq) Calculate the following for…

A: Given,   2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq)   We need to Calculate the following for the…

Q: Calculate the non-standard cell potential (in V) for the following reaction at 28.06 °C with the…

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Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A: equilibrium reaction is  Sn+2(aq) + 2 Fe+3(aq)   <-->  Sn+4(aq)   + 2 Fe+2(aq)  (1)…

Q: The free energy

A:

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

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Q: Calculate the standard free-energy change, in kilojoules, at 25 °C for the reaction 2 Ag* (aq) + Zn…

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Q: What is the maximum work (in kJ) you can obtain from 18.2 g of nickel in the following cell when the…

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Q: Consider the following galvanic cell: Li (s) | 0.095M LICI (aq) || 0.032M Sn(NO3)2 (aq) | Sn (s)…

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Q: The free energy change for the following reaction at 25 °C, when [Ag+] = 1.13 M and [Fe2+] =…

A:

Q: 33M.  I need to calculate Gibb's free energy and equilibrium constant, K.  Is the reaction…

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Q: The free energy change for the following reaction at 25 °C, when [H*] = 3.34x103 M and [Hg2*] = 1.15…

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Q: What is the cell potential (E0) for a galvanic cell formed from the following two half-reactions?…

A:

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

A: We have given that    the balanced chemical equation                    Cl2  + 2Br-  → Br2  + 2Cl-…

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.