Predict whether the following reactions will be spontaneous in acidic solution under standard conditions: (a) oxidation of Sn to Sn2+ by I2 (to form I -), (b) reduction of Ni 2+ to Ni by I - (to form I2), (c) reduction of Ce4+ to Ce3+ by H2O2, (d) reduction of Cu2+ to Cu by Sn2+ (to form Sn4+)

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Q: Molten RbCI can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

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Q: At a temperature of 298 K, the enthalpy change for the reaction A + B → C + D is -12000 J / mol and…

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Q: Molten ScCl3 can be electrolyzed to form metallic Sc For what duratiom should an electrolysis be…

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Q: Predict whether the following reactions will be spontaneousin acidic solution under standard…

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Q: cell potential

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

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Q: An aqueous solution of an unknown salt of ruthenium Is electrolyzed by a current of 2.70A passion…

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Q: Consider the following reaction and its Δ?∘Δ⁢G∘ at 25.00 °C. Fe2+(aq)+Zn(s)⟶Fe(s)+Zn2+(aq)Δ?∘=−60.73…

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Q: Calculate the equilibrium constant, K for the reaction at 298 K,Zn (s) + Cu2+(aq) ——–>  Zn2+(aq)…

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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.