ISSN:
0538-8066
Keywords:
Chemistry
;
Physical Chemistry
Source:
Wiley InterScience Backfile Collection 1832-2000
Topics:
Chemistry and Pharmacology
Notes:
A kinetic study of base-catalyzed hydrolysis of Cu(II)-malonamide complex has been performed in sodium hydroxide solution (0.2-1.25M). The reaction follows an irreversible first-order consecutive path: \documentclass{article}\pagestyle{empty}\begin{document}$$ {\rm Cu}\left({{\rm II}} \right) - {\rm Malonamide\,Complex}\mathop {\longrightarrow}\limits_{ - {\rm NH}_3 }^{k_{1obs} } {\rm Malonamic\,Acid}\mathop {\longrightarrow}\limits_{ - {\rm NH}_3 }^{k_{2obs} } {\rm Malonic\,Acid} $$\end{document} The variation of k1obs and k2obs with alkali concentration was found to be in good agreement with the equations: \documentclass{article}\pagestyle{empty}\begin{document}$$ \begin{array}{*{20}c} {1/k_{{\rm 1obs}} = B_1 + B_2 /[{\rm \bar OH]}} & {{\rm and}} \\ \end{array} $$\end{document} \documentclass{article}\pagestyle{empty}\begin{document}$$ 1/k_{{\rm 2obs}} = C_1 + C_2 /[{\rm \bar OH]} $$\end{document} where B1, B2, C1, and C2 are empirical constants. The mechanism of hydrolysis of Cu(II)-malonamide complex has been discussed and rate equations have been derived. Retardation of rate of hydrolysis due to coordination of Cu(II) with malonamide, in alkaline medium, has been explained in terms of comparatively slow breakdown of the C—N bond of the tetrahedral intermediate (TI). Thermodynamic parameters have also been evaluated.
Additional Material:
2 Ill.
Type of Medium:
Electronic Resource
URL:
http://dx.doi.org/10.1002/kin.550230906
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