Calculate the standard free-energy change for this reaction at 25 °C. A list of standard reduction potentials can be found in this table. 2 Au (aq) + 3Cr(s) 2 Au(s) + 3 Cr+ (aq) AG = kJ/mol

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Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2 +] = 0.887 M…

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Q: n the table of standard reduction potentials, locate the half-reactions for the reductions of the…

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Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.876 M and…

A: Cr(s)+Fe+2 (aq )<==>  Cr+2 (aq)+Fe(s) [Cr+2] = 0.876 M [Fe+2] = 0.0120 M

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Q: Calculate the standard free-energy change for this reaction at 25 °C. A list of standard reduction…

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A: Ga/Ga+3∥Ag+/AgE0Ga+3/Ga=-0.56 V (anode)E0Ag+/Ag=+0.80 V (cathode)E0cell =E0c-E0A=0.80-(-0.56) =+1.36…

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Q: Calculate the standard free-energy change for this reaction at 25 °C. A list of standard reduction…

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Q: Calculate the standard free-energy change for this reaction at 25 °C. A list of standard reduction…

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Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg? +] = 0.788 M…

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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.