2. Consider the Latimer diagram for phosphorus in acidic and basic solutions at 25 °C. Acidic solution H3PO4 -0.93 Basic solution PO ³- H4P₂06 -0.28 x a HPO3²- -1.35 H3PO3 -1.49 -1.57 b H₂PO₂ H₂PO₂ -0.50 y -0.51 -1.18 P -0.06 PH3 PH3 Complete the missing standard reduction potentials (a, b and c) for the Latimer diagram in acidic solution. B. Complete the missing standard reduction potentials (x, y and z) for the Latimer diagram in basic solution. C. Consider the redox reaction shown below in basic solution at 25 °C. HPO3² (aq) + PH3(g) ⇒ 2 P(s) + 2 OH (aq) + H₂O(1) (i) Write the balanced equation for the cathode half-reaction and calculate the Eºred- (ii) Write the balanced equation for the anode half-reaction and calculate the Eºox- (iii) Calculate the Eᵒcell and AG for the given redox reaction.

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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.