Consider conditions where [Fe2+]0 = 1.00 × 10–3 M, [MnO4–]0 = 0.100 M, [Mn2+]0 = 0.100 M, and the initial pH = 5.00 at 275 K. Calculate the cell potential (Ecell in V) and ΔG (in kJ/mol) for the reaction under these conditions. 5 Fe (s) + 2 MnO4– (aq) + 16 H+ (aq) → 5 Fe2+ (aq) + 2 Mn2+ (aq) + 8 H2O (l) (equation is at equilibrium) standard reduction for Fe (s) to Fe2+ is .44  standard reduction potential for MnO4- to Mn2+ is 1.51

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: Physical constants that you may need: R = 8.31446 mol K C Faraday's constant F= 96485 mol e Gas…

A: Using Nernst's equation, pH of the solution can be determined from Ecell.

Q: Calculate the cell potential of a cell operating with the following reaction at 25°C in which…

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Q: The following galvanic cell is constructed at 273 K. Each aqueous phase reactant and product has a…

A: graphite(s) | X2 (g) | XO4- , H+ || YO3-, YO2- , H+ | graphite(s)

Q: The equilibrium constant, K, was found to be 3.8 x108 at 25°C for the following reaction, 2X(s) +…

A: For the given reaction:  2X(s) +  3Y2+(aq)  →2X3+  + 3Y(s) As the charges are equal on both sides.…

Q: Consider a galvanic cell with the following components: A platinum electrode in 0.20 M Fe2+ (aq) and…

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Q: The standard reduction potential of the Pb2+/Pb electrode is -0.13 V and the standard cell potential…

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Q: Write the net cell equation for this electrochemical cell. Phases are optional. Do not include the…

A: In this electrochemical cell of cobalt metal acts as a anode and silver metal is acts as a cathode.…

Q: Like equilibrium constants, Eo cell  values are temperature dependent. At 80°C, Eo cell for the cell…

A: Given : Eo cell = 0.18 V Since nFEo cell = RT ln(K)  where n = number of electrons involved in the…

Q: A current of 0.452 A is passed through an electrolytic cell containing molten CaCl2 for 1.50 hours.…

A:

Q: The equilibrium constant, K, was found to be 2.5 x108 at 25°C for the following reaction, 2X(s) +…

A:

Q: The following cell has a potential of 0.10 V at 25oC. Ni(s) | Ni2+(aq) (1.0 M) || H+ (? M) | H2(g)…

A: Ni(s)   +    2 H+(aq)     ⇔    Ni+2(aq)   +     H2 (g)    Ecello = 0.23…

Q: Calculate the non-standard cell potential (in V) for the following reaction at 190.51 ℃ with the…

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Q: Calculate the non-standard cell potential (in V) for the following reaction at 33.56 ℃ with the…

A: The cell reaction taking place is given as, => Pb2+ (aq) + Li (s) ------> Pb (s) + Li+ (aq)…

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

A:

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

A: Answer :----- Given :---- [Cd2+ ] = 0.00100 M[Au3+ ] = 0.784 MThe overall balanced reaction are…

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

A: 1. Cl2  +  Br- -> Cl-   +    Br2 For the above reaction, At anode :      2Br-→Br2  +  2e-…

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + Co² (aq) Ti² (aq) +…

A: Cell potential of any complete cell can be measured by Nernst equation. This question will be solved…

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

A:

Q: Calculate ΔG° for the electrochemical cell Pb(s) | Pb ⁺²(aq) || Fe ⁺³(aq) | Fe ⁺²(aq) | Pt(s) A)…

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

A:

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

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Q: Calculate the cell potential and the equilibrium constant for the following reaction at 298 K:…

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Q: Consider the following electrochemical cell: Cd(s) | Cd2+ (aq) || Ce4+ (aq), Ce3+ (aq) | Pt(s) Which…

A: Nernst equation gives the relation between cell potential, standard cell potential and the…

Q: The cell potential (Ecell) of a galvanic cell made using the redox couples H+/H2 and Zn2+/Zn is…

A:

Q: Consider the following electrochemical cell: Cd(s) | Cd2+ (aq) || Ce4+ (aq); Ce³+ (aq) | Pt(s) Which…

A: In voltaic cell, The metal electrode which has higher reduction potential acts as cathode and metal…

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

A:

Q: 1) The standard reduction potentials of Cu2+ (aq) Cu(s) and Ag+ (aq) Ag(s) are +0.34 and +0.80 V,…

A: Calculate the cell potential of the given galvanic cell.  Given  At Anode  Cu/Cu2+; E°=-0.34 V At…

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

A: In an electrochemical cell, oxidation occurs at the anode and reduction occurs at the cathode. In…

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.