Protein film cryovoltammetry: Demonstrations with a 7Fe ([3Fe-4S] + [4Fe-4S]) ferredoxin

Chemical Communications

Volumn , Issue 17, 1999, Pages 1635-1636

  McEvoy, James P ^a   Armstrong, Fraser A ^a  

^a UNIVERSITY OF OXFORD   (United Kingdom)

Author keywords

[No Author keywords available]

Indexed keywords

FERREDOXIN; IRON; SOLVENT; SULFUR;

ARTICLE; ENZYME ACTIVE SITE; NONHUMAN; OXIDATION REDUCTION REACTION; POTENTIOMETRY; THERMOPLASMA ACIDOPHILUM;

EID: 0033533477     PISSN: 13597345     EISSN: None     Source Type: Journal    
DOI: 10.1039/a903222c     Document Type: Article

References (30)

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24. S. J. George, A. J. M. Richards, A. J. Thomson and M. G. Yates, Biochem. J., 1984, 224, 247; M. K. Johnson, D. E. Bennett, J. A. Fee and W. V. Sweeney, Biochim. Biophys. Acta, 1987, 911, 81; P. J. Stephens, G. M. Jensen, F. Devlin, T. V. Morgan, C. D. Stout and B. K. Burgess, Biochemistry, 1991, 30, 3200; C. D. Stout, J. Biol. Chem., 1993, 268, 25 920; Z. G. Hu, D. Jollie, B. K.Burgess, P. J. Stephens and E. Münck, Biochemistry, 1994, 33, 14 475.
25. S. J. George, A. J. M. Richards, A. J. Thomson and M. G. Yates, Biochem. J., 1984, 224, 247; M. K. Johnson, D. E. Bennett, J. A. Fee and W. V. Sweeney, Biochim. Biophys. Acta, 1987, 911, 81; P. J. Stephens, G. M. Jensen, F. Devlin, T. V. Morgan, C. D. Stout and B. K. Burgess, Biochemistry, 1991, 30, 3200; C. D. Stout, J. Biol. Chem., 1993, 268, 25 920; Z. G. Hu, D. Jollie, B. K.Burgess, P. J. Stephens and E. Münck, Biochemistry, 1994, 33, 14 475.
26. E. Laviron, in Electroanalytical Chemistry, ed. A. J. Bard, Marcel Dekker, New York, 1982, 12, 53.
27. -1) was present as co-adsorbate in both the aqueous electrode-coating solution and the cryosolvent cell solution (usually 70% v/v methanol; Prolabo > 99%) with 0.1 M NaCl buffered by HEPES at pH* 7.4 or acetate at pH* 5.0. The aqueous saturated calomel reference electrode (SCE) with internal salt bridge was held in a Luggin side arm filled with cryosolvent but maintained at room temperature with a water jacket. Values of pH and pH* [see: ref. 3(a), and R. G. Bates, Determination of pH: Theory and Practice, Wiley, New York, 1973] were measured with glass pH electrode at 273 K, without corrections. Cell anaerobicity was maintained by purging with Ar. Temperatures were controlled by immersing the cell compartment in a stirred ethanol bath, to which was added dry ice or frozen ethanol, and measured (±1 K) with a thermometer after 10 min equilibration. Background currents were subtracted using an in-house analysis program (Dr H. A. Heering).
28. o/ varies trivially as a result of pH* changes. Values obtained were: at 273 K (aqueous) pK = 5.6, at 273 K (70% v/v methanol) pK = 6.7, at 198 K (70% v/v methanol) pK = 6.8 (an apparent value since pH* is measured at 273 K).
29. The peak broadening observed as the temperature is lowered is not due to increased uncompensated resistance (iR); like irreversible electrode kinetics, iR effects are associated with large increasaes in peak separation. See: L. Roullier and E. Laviron, J. Electroanal. Interfacial Electrochem., 1983, 157, 193.
30. Peak potentials were completely restored although peak areas were ca. 10% smaller than measured at the start of the experiment.