알칼리 수용액에서 이가철 이온이 용존산소에 의하여 산화되는 산화속도를 초기농도 측정법에 따라 측정하여 반응차수를 구하고 산화반응기구를 추정하였으며 활성화에너지를 구하였다. 각각의 농도에 대한 산화반응차수는 이가철 이온농도에 대하여 1차였으며, 알칼리농도에 대한 반응차수는 알칼리농도가 0.025 mole/l부근에서 양의 차수에서 음의 차수로 변화되는 변곡점이 있음을 알았다. 용존산소에 의한 제일철의 산화반응속도식은 30 ℃ 이하에서-d[O₂]/dt=k[Fe^II][OH^-]^½[O₂]^¾/K_FeOH++[OH^-]） 이였고 40 ℃에서 -d[O₂]/dt=k"[Fe^II][OH^-][O₂]^1/2
/（K_FeOH++[OH^-]） 로 나타낼 수 있었으며 산화에 필요한 활성화에너지는 6.8 Kcal/mole이었다. 본 연구에서 제일철 이온의 산화생성물은 무정형 함수산화철인 δ-FeOOH임을 X-선회절 및 IR로서 확인하였다.

The kinetics for the oxidation reaction of ferrous ion in alkaline solution in with the dissolved oxygen was determined using initial rate method. The oxidation was conducted by injecting the ferrous ion into NaOH solution and the reaction orders in terms of oxygen consumption were the first order with respect to the ferrous ion concentration but varied with the alkali and the dissolved oxygen concentration. The deflection of reacion order with respect to alkali concentration was found to occur near 0.025 mole/l NaOH concentration. The rate equations for the oxidation were two types according to the temperature level ; one of these was -d[O₂]/dt=k[Fe^II][OH^-]^½/[O₂]^¾/K_FeOH⁺+[OH^-]） bellow 30 ℃ and another -d[O₂]/dt=k"[Fe^II][OH^-][O₂]^1/2/（K_FeOH⁺+[OH^-]) at 40 ℃. The activation energy for the oxidation of ferrous ion was 6.8 Kcal/mole. Amorphous iron oxy-hydroxide(δ-FeOOH) which had produced as reacting the iron sulfate to the NaOH in the aforementioned solution was confirmed by the X-ray diffractometer and the IR spectrophotometer.