Experimental Approach to ElectrochemistryWiley, 1977 - 211 pagine |
Dall'interno del libro
Risultati 1-3 di 33
Pagina 27
... less than 0.5 V , is negligibly slow . That is , Co , Ni , Sn , Pb and Cd fail to produce H2 from 1 M acids at 298 K. Conversely , hydrogen does not displace metals such as copper from their salts under normal circumstances , though ...
... less than 0.5 V , is negligibly slow . That is , Co , Ni , Sn , Pb and Cd fail to produce H2 from 1 M acids at 298 K. Conversely , hydrogen does not displace metals such as copper from their salts under normal circumstances , though ...
Pagina 62
... less than the back e.m.f. E 。. ( c ) The imposed current + I or load - I versus E If there are products of electrolysis they are , at least in principle , capable of recombining and acting as the reactants of a galvanic cell . The cell ...
... less than the back e.m.f. E 。. ( c ) The imposed current + I or load - I versus E If there are products of electrolysis they are , at least in principle , capable of recombining and acting as the reactants of a galvanic cell . The cell ...
Pagina 97
... less than about 0.5 V apart , then ( i ) the predicted reaction will not be complete and ( ii ) its reverse , predicted not to occur , may occur to a measurable extent . In our examples above , Fe3 + will indeed be reduced by I , but ...
... less than about 0.5 V apart , then ( i ) the predicted reaction will not be complete and ( ii ) its reverse , predicted not to occur , may occur to a measurable extent . In our examples above , Fe3 + will indeed be reduced by I , but ...
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+