By Bard A.J., Stratmann M., Scholz F.
Electrochemical tactics play an more and more huge function in our day-by-day lives; even if in generating or saving power, rust safeguard or nerve stimuli in bodies. This 11-volume encyclopedia presents either a simple creation to all themes on the topic of smooth electrochemistry in addition to finished evaluation of the topic. Unrivalled in its breadth and intensity, this top notch reference paintings has been created and written via popular scientists, masking every thing from basic study to components of program.
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Additional resources for Encyclopedia of Electrochemistry, Inorganic Chemistry
70. 8 kJ mol−1 . 3, 2963 kJ mol−1 . 6, 2704 kJ mol−1 . 4, 1971, 2878 kJ mol−1 . 7 kJ mol−1 . 02 V (The electrode reactions of these compounds are highly irreversible, therefore, 53 54 2 Standard, Formal, and Other Characteristic Potentials of Selected Electrode Reactions practically all E 0 values are calculated from caloric data. 6994 V (There are several carbon compounds that exhibit reversible behavior. 172 g. 4 kJ mol−1 . 495 V The E 0 values were calculated from thermodynamic data. There are a large number of different acids, especially of the polyacid type.
3 kJ mol−1 . 3 kJ mol−1 . 77 × 10−14 Complex equilibria Recent data on several Pb2+ complexes can be found in Refs 59, 64. 00677 N), OS: +5, +4, +3, +2, +1, 0, −1/3, −1, −2, −3; IE: 1402, 2856, 4577 kJ mol−1 , 16 920 (IV + V) kJ mol−1 . 1 V (Nitrogen ﬁxation, that is, the conversion of N2 to the nonzero OS, is thermodynamically possible; however, both the oxidation and the reduction of N2 are kinetically hindered. 324 × 10−3 g. Solubility of ammonia in 100 g water at 1 bar and 20 ◦ C is 54 g. 9739 15 P), OS: +5, +4, +3, +2, +1, 0, −1/3, −1, −2, −3; IE: 1402, 2856, 4577 kJ mol−1 , 16920 (IV + V) kJ mol−1 .
98 83 Bi), OS: +5, +3, 0, −3; IE: 703, 1610, 2466 kJ mol−1 , 9776 (IV + V) kJ mol−1 . 5 kJ mol−1 . 42 × 10−3 g. 3 kJ mol−1 , EA: 200 and −414 kJ mol−1 . 66 V The standard potentials of sulfur compounds are mostly calculated thermodynamically because the redox systems – except that of sulﬁte–dithionite – are irreversible. In excess sulﬁde, sulfur dissolves in the form of polysulﬁdes.