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i 1 Ge010giu(Tecknus Inc Page 2 Addendum-Feasibility Study Project No 507 2 January 15,2003 ' has been depleted by this reaction and mineral compounds, such as Mn02, NO3, Fe(0)31 SO4 and H+,become the e donor (listed in decreasing Eh values) Table 1 below lists the common Redoxotential and relative oxidizing ower of the P g P ' primary oxidants According to the RWQCB, infection of ozone, peroxide and oxygen are acceptable agents to use without needing a waste discharge requirement permit Therefore, these are the three agents we have proposed to use ' Table 1. Comparison of relative strength of oxidants Std. Redox Potential Relative Oxidizing Oxidant E° (Volts) Power' Fluorine (F.) 30 223 Hydroxyl Radical (OH) 28 206 ' Oxygen Radical CO) (Superoxide) 24 1 76 Ozone (03) 2 1 1 54 ' Hydrogen Peroxide (11202) 1 8 1 31 Permanganate (Mn04) 1 7 1 24 Chlorine Dioxide (C102) 1 6 1 15 Chlorine (C12) 1 4 1 00 Oxygen (OZ) 12 086 Bromine (Br.) 1 1 080 ' Iodine (1.) 08 054 1 =Normalized to Chlorine,where C1,= 1 0 Listed below are selected reaction and the volume of oxidant needed to destroy one pound of MTBE We recognize that the J M Equipment site in Stockton contains MTBE at low concentration and that the BTEX and TPH-G are the primary compounds to be mitigated, rbut this table gives a guide for the type of reaction and the volumes of oxidants needed From a stoichiometric reaction standpoint, the oxidation of BETX should take approximately the same volume of peroxide as MTBE since there are a similar number of carbons in both molecules BTEX actually has more, but MTBE bonds are harder to break Gasoline range hydrocarbons, known as paraffins or alkanes, have similar numbers of carbon atoms as the aromatic hydrocarbons (or arenas) and MTBE, and therefore should require a similar volume of peroxide to oxidize