Tuesday 20 March 2018 photo 15/15
![]() ![]() ![]() |
Reduction potential table pdf: >> http://zlp.cloudz.pw/download?file=reduction+potential+table+pdf << (Download)
Reduction potential table pdf: >> http://zlp.cloudz.pw/read?file=reduction+potential+table+pdf << (Read Online)
Table of Standard reduction potentials www.vaxasoftware.com. Half reaction ?o. (V). Li. +. + e. ? > Li(s). ?3.0401. +REDUCING. K+ + e. ? > K(s). ?2.931. Ca2+ + 2e. ? > Ca(s). ?2.868. Na+ + e. ? > Na(s). ?2.7144. Mg2+ + 2e. ? > Mg(s). ?2.3568. Al3+ + 3e. ? > Al(s). ?1.676. Mn2+ + 2e. ? > Mn(s). ?1.185. 2H2O + 2e.
Standard Reduction Potentials of Half-Cells. (Ionic concentrations are at 1M in water @ 250 C). Oxidizing Agents. Reducing Agents. E0 (Volts). F2(g) + 2e-. 2F-(aq). +2.87. PbO2(s) + SO4. 2-(aq) + 4H+(aq) + 2e-. PbSO4(s) + 2H2O(и). +1.69. >. MnO4. -(aq) + 8H+(aq) + 5e-. Mn2+(aq) + 4H2O(и). +1.51. >. Au3+(aq) + 3e-.
Standard Reduction Potentials at 25°C (298K). Half-Reaction. E°(V). F2(g) + 2e- > 2F-(aq). +2.87. Co3+(aq) + e- > Co2+(aq). +1.81. H2O2(aq) + 2H+(aq) + 2e- > 2H2O(l). +1.78. PbO2(s) + HSO4. -(aq) + 3H+(aq) + 2e- > PbSO4(s) + 2H2O(l). +1.69. Au+(aq) + e- > Au. +1.69. Pb4+(aq) + 2e- > Pb2+(aq). +1.67. 2HClO(aq)
17 and 25. 1964 and 1971); G. Milazzo and S. Caroli, Tables of Standard Electrode Potentials (New York: Wiley, 1978); T. Mussini, P. Longhi, and S. Rondinini, Pure Appl. Chem. 1985, 57, 169. Another good source is A. J. Bard, R. Parsons, and J. Jordan. Standard Potentials in Aqueous Solution (New York: Marcel Dekker,
Table of Standard Reduction Potentials. Cathode (Reduction). Half Reaction Standard. Potential E o. (V). Li+ (aq) + e- > Li (s). -3.0401. Cs+ (aq) + e- > Cs (s). -3.026. Rb+ (aq) + e- > Rb (s). -2.98. K+ (aq) + e- > K (s). -2.931. Ba2+ (aq) + 2 e- > Ba (s). -2.912. Sr2+ (aq) + 2 e- > Sr (s). -2.89. Ca2+ (aq) + 2 e- > Ca (s).
Reduction Half–Reaction. Eo(V). F2(g) + 2e– > 2F–. (aq). 2.86. OF2(g) + 2H+. (aq)+ 4e– > H2O(l) + 2F–. (aq). 2.1. O3(g) + 2H+. (aq)+ 2e–. > O2(g) + H2O(l). 2.075. S2O8. 2–. (aq) + 2e–. > 2SO4. 2–. (aq). 2.01. Ag2+. (aq) + e–. > Ag+. (aq). 1.98. Co3+. (aq) + e–. > Co2+. (aq). 1.82. H2O2(aq)+ 2H+. (aq)+ 2e–. > 2H2O(l).
There are three tables for this electrochemical series . Each table lists standard reduction potentials, E° values, at 298 .15 K (25 °C), and at a pressure of 101 .325 kPa (1 atm) . Table 1 is an alphabetical listing of the elements, according to the symbol of the elements . Thus, data for silver (Ag) precede those for aluminum (Al)
STANDARD REDUCTION POTENTIALS IN AQUEOUS SOLUTION AT 25°C. Half-reaction. E°( )V. 2. F ( ) 2 g e. -. +. 3+. -. ?. 2 F. 2+. -. 2.87. Co e. +. ?. Co. 1.82. 3+. -. Au. 3 e. +. ?. Au( )s. 1.50. 2. Cl ( ) 2 g e. -. +. +. ?. 2 Cl. -. 1.36. 2. O ( ) 4H. 4 g e. -. +. +. ( )l e. -. ?. 2. 2H O. -. 1.23. 2. Br ( ) 2 l e. -. +. ?. 2 Br. 2+. 1.07. 2+.
There are three tables for this electrochemical series. Each table reliability. The values of reduction potentials, in particular those. |lists standard reduction potentials, E° values, at 298.15 K (25 °C), of less common reactions, are not definite; they are subject to oc- and at a pressure of 101.325 kPa (1 atm). Table 1 is an
STANDARD REDUCTION POTENTIALS FOR HALF-REACTIONS. Ionic concentrations are a 1 M in water at 25°C. Half-reaction. E° (Volts). F2(g) + 2e- > 2F- +2.87. H2O2 + 2 H+ + 2e- > 2 H2 .. +1.77. MnO4. - + 8 H+ + 5e- > Mn2+ + 4 H2O .
Annons