Luo Fang-xiang
2010
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Journal
Journal of Nuclear and Radiochemistry
Abstract
The reaction kinetics between HNO2 and formaldoxime in perchloric acid media were studied by spectrophotometric method.The reaction rate equation was determined as follows:-dc(HNO2)/dt=kc(HNO2)c1.32(FO)c0.96(ClO-4),where k=(7.55±0.50)(mol/L)2.28/s at 1.0 ℃.The reaction activation energy Ea is(65.16±6.52) kJ/mol.Effects of c(FO),c(H+),c(ClO-4) and temperature on the reduction rate of HNO2 were investigated.HNO2 can be rapidly reduced by FO under usual conditions.The reaction rate increased while increasing concentration of FO,ClO-4 and reaction temperature.However,the influence of H+ is negligible.