Sulfur, with an atomic weight of 32.06, has four stable isotopes. By far the most abundant is 32S, representing around 95% of the total sulfur on Earth. The next most abundant isotope is 34S, followed by 33S, and finally 36S is the least abundant contributing only 0.0136% to the total (Table 11). The natural abundances of sulfur isotopes, however, vary from these values as a result of biological and inorganic reactions involving the chemical transformation of sulfur compounds. For thermodynamic reasons, the relative abundance of sulfur isotopes can vary between coexisting sulfur phases. This...

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