Consider the reaction, 2 Al(s) + 3 I2(s) → 2 Al3+(aq) + 6 I–(aq), which can be obtained with the following two half reactions: Al3+(aq) + 3 e– → Al(s), E°red = –1.66 V I2(s) + 2 e– → 2 I–(aq),  E°red =  0.54 V At 25 °C and a concentration of I–(aq) of 0.15 M, the measured cell potential is 2.32 V. What was the concentration of Al3+(aq) under these conditions?

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A: Solution -

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Q: half-reaction standard reduction potential MnO,(aq)+2H,0(1)+3e MnO,(s)+4 OH (aq) E=+0.59 V red 2+…

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Q: The solubility product for CuI (s) at 25.0 °C is 1.1 × 10−12 M2. Calculate the value of E°red at…

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Q: E°cell

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Q: Consider the following half-reactions: E° = +2.87 V F2(9) + 2 e ® 2 F'(aq) Cu2*(aq) + 2 e¯ ® Cu(s)…

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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.