Consider the following reactions. Are they spontaneous in the direction written, under standard conditions at 25°C? Standard electrode potentials in aqueous solution at 25°C ar Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Standard Cathode (Reduction) Half-Reaction Potential, E (V) Cu+ (aq) +e Cu* (aq) 0.16 Fe+ (aq) + e Fe?+ (aq) 0.77 O2 (9) + 4H (ag) + 4e 2H20(1) MnO, (ag) + 8H (aq) + 5e - Mn2+ (ag) + 4H2O(1) 1.49 1.23 a. Cu?+ (ag) + Fe2+ (ag) → Cu* (aq) + Fe+ (ag) spontaneous O nonspontaneous b. 4MNO, (ag) + 12H+ (ag) → 4MN²+ (aq) + 502 (9) + 6H2O(1) O spontaneous Ononspontaneous

Q: 3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) What would be the pH of…

A: Given cell reaction: 3Co(s)+2NO3-(aq)+8H+→3Co+2(aq)+2NO(g)+4H2O(l)

Q: Consider the following cell notation : Cr (s) |Cr^ 3+ (aq)||H 3 AsO 4(aq) ,H^ * (aq),H 3 AsO 3(aq)…

A: In the cell notation, the left most part indicates anode. At anode oxidation takes place. After the…

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

A:

Q: Given the standard cell potential, E°ce = 1.10 V, for the cell, Zn(s) | Zn(NO,)(aq) || Cu(NO,)(aq) |…

A: Standard cell potential (E°cell) = 1.10 V  Temperature = 25°C.  The reaction :  Zn(s) + Cu2+(aq)…

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: A constant current flows for 3.75 h through an electrolytic cell containing aqueous AgNO3(aq).…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: Predict the standard potential for the galvanic cell. Refer to the table of standard reduction…

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Q: An electrochemical cell Bi(s) | Bi2S3(s) | Bi2S3(aq) | Bi(s) the standard potential is 0.96 V at 25…

A: we  have to calculate the equilibrium constant for the cell

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

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Q: Calculate the free energy for a spontaneous galvanic cell where the standard half-cell potentials…

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

A:

Q: Given the reaction    4 Al(s) + 3O2(g) ===>  2Al2O3(s), write the half reactions and calculate…

A: The reaction given is, => 4 Al (s) + 3 O2 (g) --------> 2 Al2O3 (s)

Q: The cell potential of the following electrochemical cell is determined by using an unspecified…

A: We have find out the answer.

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

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Q: Calculate the equilibrium constant K for the following reaction at 25°C from standard electrode…

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Q: The reaction Sn (s) + 2 Cu²+ (aq) = Sn²+ (aq) + 2 Cu+ (aq) has a standard potential of 0.29 V at 25…

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Q: Consider the following galvanic cell reaction at 25 oC, 4 Cr2+(aq) + O2(g) + 4 H3O+(aq) → 4 Cr3+(aq)…

A: Nernst equation: The Nernst equation relates to the reduction potential of an electrochemical…

Q: Consider the following galvanic cell at 25°C:Pt|Cr2+(0.30M),Cr3+(2.0M)||Co2+(0.20M)|CoThe overall…

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

A: The electromotive force (emf) or voltage of an electrochemical cell when it is not in its normal…

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

A:

Q: 1 Calculate the standard free energy change for the fol- lowing reactions using the standard cell…

A: Standard free energy change is as follows:∆G∘=-nFEcell∘Where n is number of electron transfer…

Q: Consider the following galvanic cell and calculate the cell potential (Ecell). Co(s) | Co2"(aq, 0.15…

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Q: 3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) Determine the cell…

A: Given cell reaction:

Q: Half-Reaction F(g) + 2e™ - +2F (aq) O(g) + 2H*(aq) + 2e. Co (aq) + e- H₂O(aq) + 2H*(aq) + 2e Cu²+…

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Q: For the cell reaction, Zn(s) | Zn2*(aq, 1 M) || Cu2*(aq, 1 M) | Cu(s), the electrode potential of…

A: Cell Notation :  Zn(s) | Zn2+(aq,1M) || cu2+(aq, 1M) | Cu(s)  Electrode potential of cathode = 0.34…

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

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Q: sing the following standard reduction potentials E° = -2.92 V Cs*(aq) + e¯ 2*(aq) + 2 e¯ → Cs(s) E°…

A: In a cell, there are two components. One is anode and oxidation takes place at this component.…

Q: Calculate the cell potential for the galvanic cell in which the reaction Al(s) + Au³(aq) Al³(aq) +…

A: The reaction :

Q: Use the biological standard potentials of two reduction reactions 4H* + 4e + 02-> 2 H20, E = + 0.82…

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Q: Consider the following reaction and its AG at 25.00 °C. Fe2+(aq) + Zn(s) – Fe(s) + Zn?+(aq) AG' =…

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Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

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Q: For the cell shown, the measured cell potential, Ecell, is −0.3627 V at 25 °C. Pt(s) | H2(g,0.735…

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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.