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HWAHAK KONGHAK,
Vol.34, No.2, 249-252, 1996
Vol.34, No.2, 249-252, 1996
수용액상에서 과산화수소의 분해
Decomposition of Hydrogen Peroxide in the Aqueous Solution
수용액상에서 과산화수소의 분해반응이 온도 70, 80, 90℃, 질산농도 0-4M 범위에서 수행되었다. 분해반응은 과산화 수소에 대하여 1차반응이었으며, 질산농도가 2M 이상에서 산촉매 현상에 의해 반응속도는 증가되었다. 속도식은 다음과 같다.
ln[H2O2]/[H2O2]o = -2.23×1010 exp(-18200/RT)ㆍt ([H+]<2M)
ln[H2O2]/[H2O2]o = -[2.23×1010 exp(-18200/RT)+2.1×1012 exp(-21200/RT)([H+]-2)]ㆍt([H+]>2M)
또한 UO2+2, Nd+3, Fe+3, MoO2+2, Sr+2, Cs+1 같은 금속이온들이 수용액상에서 과산화수소의 분해에 미치는 영향이 조사되었으며 이들 분해속도는 금속이온이 함유되지 않은 수용액상에서의 분해속도와 비교되었다.
ln[H2O2]/[H2O2]o = -2.23×1010 exp(-18200/RT)ㆍt ([H+]<2M)
ln[H2O2]/[H2O2]o = -[2.23×1010 exp(-18200/RT)+2.1×1012 exp(-21200/RT)([H+]-2)]ㆍt([H+]>2M)
또한 UO2+2, Nd+3, Fe+3, MoO2+2, Sr+2, Cs+1 같은 금속이온들이 수용액상에서 과산화수소의 분해에 미치는 영향이 조사되었으며 이들 분해속도는 금속이온이 함유되지 않은 수용액상에서의 분해속도와 비교되었다.
The Kinetics of the decomposition of H2O2 in the acidic solution was investigated. The investigation was conducted within the range of HNO3 concentration of 0-4 M at temperature of 70, 80 and 90℃, respectively. The decomposition reaction is first order with respect to [H2O2] and is enhanced by acid-catalytic effect above HNO3 of 2 M. The rates are as follows;
ln[H2O2]/[H2O2]o = -2.23×1010 exp(-18200/RT)ㆍt ([H+]<2M)
ln[H2O2]/[H2O2]o = -[2.23×1010 exp(-18200/RT)+2.1×1012 exp(-21200/RT)([H+]-2)]ㆍt([H+]>2M)
The effect of UO2+2, Nd+3, Pd+2, Fe+3, MoO2+2, Sr+2, and Cs+ on the decomposition of H2O2 in the solution were examined too, and rate was compared with that obtained from metal ion-free solution.
ln[H2O2]/[H2O2]o = -2.23×1010 exp(-18200/RT)ㆍt ([H+]<2M)
ln[H2O2]/[H2O2]o = -[2.23×1010 exp(-18200/RT)+2.1×1012 exp(-21200/RT)([H+]-2)]ㆍt([H+]>2M)
The effect of UO2+2, Nd+3, Pd+2, Fe+3, MoO2+2, Sr+2, and Cs+ on the decomposition of H2O2 in the solution were examined too, and rate was compared with that obtained from metal ion-free solution.
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[Cited By]
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