Experimental Approach to Electrochemistry

AgNO3 anode Appendix aqueous solution Br₂ calculate carbon cathode cell constant cell potential cell reaction chemical Chemistry circuit Cl₂ cm² cm³ concentration cell conductimetric copper(II coulometric Cu2+ Cu²+(aq current density CuSO4 decomposition potential dilute discharge dissolved dm³ Ecell effect electricity electrochemical electrochemistry electrode potential electrode reactions electrolyte equation equilibrium equivalence point ethanoic acid Expt Fe² Fe2+ Fe³ Fe3+ free energy fuel cell galvanic cell graph H₂ H₂O half-cell half-equations half-reactions heat hydrated hydrogen hydroxide increase ionic ions lead(II measured mercury metal molar conductivity mole molecules molten NaOH negative Nernst equation overpotential oxidation oxygen plating platinum polarity potassium potential difference potentiometer reactants redox reactions reduction potentials reference electrode resistance reversible cell potential salt bridge shown in Fig silver sodium chloride soluble standard sulphate(VI sulphuric acid surface temperature theory titration transport numbers vanadium(II variation voltmeter wire zero zinc Zn2+