Experimental Approach to ElectrochemistryWiley, 1977 - 211 pagine |
Dall'interno del libro
Risultati 1-3 di 19
Pagina 108
Nicholas J. Selley. 6 Electrolysis 6.1 Minimum decomposition potentials In Chapter 4 the distinction was made between the reversible cell potential and the actual potential difference maintained by a galvanic cell in use ; and similarly ...
Nicholas J. Selley. 6 Electrolysis 6.1 Minimum decomposition potentials In Chapter 4 the distinction was made between the reversible cell potential and the actual potential difference maintained by a galvanic cell in use ; and similarly ...
Pagina 112
... minimum practical cell overpotential is not the overpotential at zero current ( which would actually be zero , see §6.2 ) , but the overpotential at low current , the current at which decomposition ... potential , for the actual ...
... minimum practical cell overpotential is not the overpotential at zero current ( which would actually be zero , see §6.2 ) , but the overpotential at low current , the current at which decomposition ... potential , for the actual ...
Pagina 132
Nicholas J. Selley. 132 Electrolysis 6.8 Summary The minimum practical decomposition potential for an electrolytic reaction is obtained by the extrapolation of the apparently straight line portion of a current / applied potential graph ...
Nicholas J. Selley. 132 Electrolysis 6.8 Summary The minimum practical decomposition potential for an electrolytic reaction is obtained by the extrapolation of the apparently straight line portion of a current / applied potential graph ...
Parole e frasi comuni
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+