Consider the following pairs of reactions: Fe2+ (aq) + 2 e- → Fe (s) E° = – 0.44 V Au3+ (aq) + 3 e-→Au (s) E° = +1.50 V Write a balanced spontaneous reaction. Calculate the standard cell potential (E°) of the cell. Calculate the cell potential (E) when [Au3+] = 0.250 M and [Fe2+] = 0.180 M. Assume standard conditions.

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: The given half-reactions are given as, Cu2+aq+e-→Cuaq    E°red=+0.153 VMnO4-aq+8H++5e-→Mn2+aq+4H2Ol…

Q: 3. A galvanic cell is constructed comprising cadmium anode and nickel cathode: Cd (s) + Ni²+ (aq) →…

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Q: Calculate the standard free energy charge for the following reactions using the standard cell…

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Q: The reaction of tin metal with acid can be written as Sn(s) +2H*(aq) → Sn²+(aq) +H2₂(g) assume…

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Q: The reaction 2Ag*(ag) + Cu(s) → 2Ag(s) + Cu2+(ag) was used in a galvanic celI. E°=0.46 V for this…

A: Given The redox reaction in the galvanic cell is as follows: 2Ag+(aq) + Cu(s)→2Ag(s) + Cu2+ (aq).…

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

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Q: For the reaction: Pd2+ + Ni → Ni²+ + Pd , AG° is –239 kJ/mole. What is the standard reduction…

A: The tendency possessed by ions to get reduced in any reaction is termed as its "standard reduction…

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

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

A: [Co2+]=0.00190 M[Au3+]=0.896 MT=25oC=25+273=298K

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)…

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: Using the following standard reduction potentials, Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V Cu2+(aq) +…

A: The standard cell potential (Eocell) for the cell is determined  using the following equation…

Q: half-reaction standard reduction potential Br,()+2e 2 Br (aq) E =+1.065 V red MnO (aq)+8H (aq)+5e Mn…

A: The half cell for which the value E°red is higher, will be preferred as the cathode. Here, MnO4-…

Q: Calculate the standard cell potential of the galvanic cell that will be produced from these two…

A: Electrochemistry is branch of chemistry in which both oxidation and reduction reaction takes place…

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

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Q: Calculate AG° and K for the following cell reactions. State whether the cell reaction is spontaneous…

A: recall the given reaction and also the values of electrode potential of the given half cell Cus +…

Q: Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe³+(aq) + B(s) + 6H₂O(1)→…

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Q: Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.29 M), Cr3+ (2.0 M) || Co 2+ (0.18 M) |…

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

A: The oxidation and reduction half cells are as follows: Oxidation: 3Ca (s) →3 Ca+2     E0= -2.87…

Q: The free energy change for the following reaction at 25 °C, when [Ag*]= 1.16 M and [Cd²+]= 3.49×10-3…

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

A: In the given galvanic cell ->Concentration of Cr3+ = [Cr3+(aq)] = 4.87 MConcentration of Ca2+ = […

Q: When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes, the…

A: 8.15mA current flows which is equal to 0.00815A time is 12.6min = 756s The molar mass of I2 =…

Q: 18) Calculate the standard cell potential for the following reaction occurring in an electrochemical…

A: Given :  18.  In the given reaction K(s) is getting oxidized while I2(s) is getting reduced.  19.…

Q: Consider the following standard reduction potentials: Al³+ (aq) + 3e-→→ Al(s), Eº = -1.66 V AgBr(s)…

A: The species which undergo oxidation and help other species to undergo reduction are called…

Q: Calculate the change in standard Gibbs energy (AC), in kilojoules, for the reaction below at 25 °C.…

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Q: 8.Using the following standard reduction potentials: Fe3+(aq) + e- → Fe2+(aq)…

A: 1) We have given the reaction as follow                          Pb2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq)…

Q: Consider the following reduction half-reactions and the corresponding standard reduction potentials,…

A: Given that : We have to rank following the reducing agents in terms of increasing strength, i.e.…

Q: Calculate E° and Ecell (at 25 °C) for the following cell reaction: Mg (s) + Sn2+ (aq) → Mg2+ (aq)…

A: Given, Sn2+ (aq) → Sn (s)             E°= ‒0.14 V Mg2+ (aq) → Mg  (s)          E°= ‒2.37 V

Q: Please don't provide handwritten solution ...

A: The objective of the question is to identify the half-reactions at the cathode and anode and…

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: Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The…

A: Eocell = 0.019 V [Zn²⁺] = 0.0223 M [Cr³⁺] = 0.1636 M The given reaction is:…

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

A: Given,

Q: Find

A: We will calculate reduction potential

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 galvanic cell was created using the following electrode reactions. Anode half-cell: Co(s) + 3…

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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.