a) Balance the following reactions.  b) Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions.  c) Identify the reactions with K > 1 among the following redox reactions.  d) Write the line representations for the Galvanic cells, indicating the anode and cathode. Cl2 +  Br- -->  Cl-   +    Br2 MnO4- +  H+  +  Ce3+  --> Ce4+  +  Mn2+  +  H2O Pb2+ -->Pb  +  Pb4+ NO3- +  H+ +  Zn  -->  Zn2+   +  NO2  +  H2O

Q: Calculate the cell potential for the galvanic cell in which the reaction   Ti(s)+Cu2+(aq)↽−−⇀…

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Q: NO3 + H* + Zn → Zn²+ + NO2 + H2O

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Q: The standard cell potential for the reaction provided below is 0.301 V, (where X is a non-metal…

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

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Q: Consider the following reaction and its AG° at 25.00 °C. Fe2+ (aq)+Zn(s) → Fe(s) + Zn²*(aq) AG° =…

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Q: Calculate the Gibbs free energy, AG°, for a galvanic cell whose two half-reactions: Mt3+ (aq) +3…

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

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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: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au³+(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.