To bet ter compare the reaction rates observed for various iron particles, it is essential to quantify the reactivity per unit metal surface area. The rate of transformation for a chlorinated organic compound in a batch system can be described by the following equation [4]: pseudo-first-order kinetics. Best-fit values of KSA are 5.31X1 O'4 for nanoscale iron and 1.0x1 O'4 for the Aldrich iron, respectively. Several factors may contribute to the difference in reactivity. Laboratory synthesized nanoscale iron surface may have “fresher” metal surface due to less surface oxidation or surface contamination. Mass transfer resistance was also less significant for the nanoscale iron batch system. The metal to solution ratio for the Aldrich iron experiment (10 g/20 mL) was 40 times of that for the nanoscale iron experiment (0.25 g/20 mL). However, the two batch systems had similar mixing intensity (mixed on a rotary shaker at 30 rpm). It was observed that most of the Aldrich iron particles were settled at the bottom of the bottle while Figure 2. Reactions of commercial grade iron particles (Aldrich, <10 pm) with CT. Initial CT concentration was 0.103 mM (15.9 mg/L). Metal to solution ratio was 10 g/20 mL.

DOI link for To bet ter compare the reaction rates observed for various iron particles, it is essential to quantify the reactivity per unit metal surface area. The rate of transformation for a chlorinated organic compound in a batch system can be described by the following equation [4]: pseudo-first-order kinetics. Best-fit values of KSA are 5.31X1 O'4 for nanoscale iron and 1.0x1 O'4 for the Aldrich iron, respectively. Several factors may contribute to the difference in reactivity. Laboratory synthesized nanoscale iron surface may have “fresher” metal surface due to less surface oxidation or surface contamination. Mass transfer resistance was also less significant for the nanoscale iron batch system. The metal to solution ratio for the Aldrich iron experiment (10 g/20 mL) was 40 times of that for the nanoscale iron experiment (0.25 g/20 mL). However, the two batch systems had similar mixing intensity (mixed on a rotary shaker at 30 rpm). It was observed that most of the Aldrich iron particles were settled at the bottom of the bottle while Figure 2. Reactions of commercial grade iron particles (Aldrich, <10 pm) with CT. Initial CT concentration was 0.103 mM (15.9 mg/L). Metal to solution ratio was 10 g/20 mL.

To bet ter compare the reaction rates observed for various iron particles, it is essential to quantify the reactivity per unit metal surface area. The rate of transformation for a chlorinated organic compound in a batch system can be described by the following equation [4]: pseudo-first-order kinetics. Best-fit values of KSA are 5.31X1 O'4 for nanoscale iron and 1.0x1 O'4 for the Aldrich iron, respectively. Several factors may contribute to the difference in reactivity. Laboratory synthesized nanoscale iron surface may have “fresher” metal surface due to less surface oxidation or surface contamination. Mass transfer resistance was also less significant for the nanoscale iron batch system. The metal to solution ratio for the Aldrich iron experiment (10 g/20 mL) was 40 times of that for the nanoscale iron experiment (0.25 g/20 mL). However, the two batch systems had similar mixing intensity (mixed on a rotary shaker at 30 rpm). It was observed that most of the Aldrich iron particles were settled at the bottom of the bottle while Figure 2. Reactions of commercial grade iron particles (Aldrich, <10 pm) with CT. Initial CT concentration was 0.103 mM (15.9 mg/L). Metal to solution ratio was 10 g/20 mL.