Mn(k) | Mn²+(0.2 M) || H+ (pH= ?) | H2 (g, 1.5 atm) | The cell potential of the Pt(k) Cell was found to be 1.04 V. Since it is known that the standard reduction electrode potential of the manganese electrode is -1.18 V, calculate the pH of the solution whose concentration is unknown.

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Q: (a) The cell potential for the following electrochemical cell at 25°C is 1.00 V. Pt(s) |H2 (g, x…

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Q: A galvanic cell was prepared by immersing an anode and a cathode of the same material (of A type) in…

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Q: Given the standard cell potential for this cell is 0.115 V, and the measured cell potential is…

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Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: Given Ecell = 0.233V Ecell = - RTnFln [H+]0.233= - 8.314 x2981 x 96500ln [H+]- 9.075 = ln [H+] [H+]…

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Q: What is the cell potential of a galvanic cell that has a reduction potential at the cathode of 0.85…

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Q: A galvanic cell is constructed in which the overall reac- tion is Brz (€) + H2(g) + 2 H20(€) → 2 Br…

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Q: Consider this galvanic cell at 298 K:                 2 Cr(s)  +  3 Ni2+(aq)      2 Cr3+(aq)  +…

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Q: The standard reduction potential (E°) for the conversion of Cr,0 to Cr* at 25°C in an aqueous…

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A:

Q: 4H* + 4e + O2 -> 2 H2O, E• = + 0.82 V NAD* + H* + 2e -> NADH, E• = -0.32 V applied to the…

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Q: For the reduction of MnO4− to Mn2+ in aqueous acid, ε⁰ = 1.51 v.For the reduction of I2 to 2I− in…

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Q: If at 25°C the standard electrode potential of the Ag/Ag' electrode is U.799 V, and the equilibrium…

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A:

Q: 11. Consider the following reaction and its AG-AG• at 25.00 °C. 2Ag(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG…

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

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Q: At 298 K a cell reaction has a standard cell potential of+0.17 V. The equilibrium constant for the…

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Q: For the following electrochemical cell: Mn(s)|Mn2+(aq)(.215M)||Cr3+(aq)(.113M),…

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A: The half reactions are  1) Mt3+ (aq) + 3 e- → Mt (s)                                Eo = 1.09 V 2)…

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.