Experimental Approach to ElectrochemistryWiley, 1977 - 211 pagine |
Dall'interno del libro
Risultati 1-3 di 25
Pagina 82
... addition would be wrong . For example : Fe → Fe2 + + 2e ; Ex = +0.44 V ( z = 2 ) Fe2 + → Fe3 ++ e ; E = -0.77 V ( z = 1 ) - >> Ex Fe → Fe3 ++ 3e ̄ ; E # −0.33 V Ox Simple addition gives an answer of -0.33 V for the third oxidation ...
... addition would be wrong . For example : Fe → Fe2 + + 2e ; Ex = +0.44 V ( z = 2 ) Fe2 + → Fe3 ++ e ; E = -0.77 V ( z = 1 ) - >> Ex Fe → Fe3 ++ 3e ̄ ; E # −0.33 V Ox Simple addition gives an answer of -0.33 V for the third oxidation ...
Pagina 152
... addition of titrant , at various total volumes . A graph of this kind could be made by plotting the slope of the ordinary titration curve ( dE / dV ) , against V. It is also possible to measure the differential potential directly , by ...
... addition of titrant , at various total volumes . A graph of this kind could be made by plotting the slope of the ordinary titration curve ( dE / dV ) , against V. It is also possible to measure the differential potential directly , by ...
Pagina 195
... addition of excess aqueous ammonia , and the acid replaced by ammonia plus ammonium sulphate solution , in order to intensify the colour of the migrat- ing copper ions . The demonstration is suitable for overhead projection . References ...
... addition of excess aqueous ammonia , and the acid replaced by ammonia plus ammonium sulphate solution , in order to intensify the colour of the migrat- ing copper ions . The demonstration is suitable for overhead projection . References ...
Sommario
1 | 8 |
The stoichiometry of electrolysis Faradays Laws | 15 |
5 | 21 |
Copyright | |
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Parole e frasi comuni
activity coefficient AgNO3 aluminium anode Appendix aqueous solution Calculate carbon cathode cell potential cell reaction chemical circuit cm² cm³ concentration cell conductimetric constant copper copper(II coulometric Cu² Cu2+ Cu²+(aq current density CuSO4 decomposition potential dilute discharge dissolved dm³ Ecell effect electricity electrochemical electrochemistry electrode potential electrode reactions equation equilibrium equivalence point ethanoic acid Fe² Fe2+ Fe³ Fe3+ free energy fuel cell galvanic cell glass electrode graph H₂ H₂O half-cells half-equations half-reactions heat hydrogen hydroxide increase iodine ionic ions measured mercury metal minimum decomposition potential molar conductivity mole NaOH negative Nernst equation overpotential oxygen plating platinum polarity potassium potential difference potentiometer reactants redox potentials redox reactions reduction potentials reference electrode resistance reversible cell potential salt shown in Fig silver sodium chloride soluble sulphate sulphate(VI sulphuric acid surface temperature titration transport numbers vanadium(II variation voltmeter zero zinc Zn2+