Recall that the hydrogen half-cell H+(aq) + e- H2(g) is assigned a standard electrode potential of zero by convention. Interpret standard electrode potential data in terms of ease of oxidation/reduction.
Recall that a standard cell potential Ecell, can be calculated from standard electrode potentials and has a positive value for a spontaneous reaction. Predict whether a reaction is spontaneous in the forward or reverse direction from Edata.
Understand that the equation G= -nFEcellshows the relationship between standard change in Gibbs energy and standard cell potential for a reaction. Determine the value for GfromEdata.
Understand that during electrolysis of aqueous solutions, competing reactions can occur at the anode and cathode. Deduce from standard electrode potentials the products of the electrolysis of aqueous solutions. Explain the effects of concentration and the nature of the electrode for electrolysis of NaCl(aq) and CuSO4(aq).
Recall that electroplating involves the electrolytic coating of an object with a metallic thin layer. Deduce equations for the electrode reactions during electroplating.