| Abstrakt: |
The kinetics of Hg(II) accelerated substitution of cyanide with isoniazid (INH) from [Ru(CN)6]4– was investigated via measurement of the rise in absorbance at 502 nm. Employing the pseudo-first-order condition, the reaction's advancement has been examined as an indicator of [Hg(II)], pH, [INH], , temperature, and ionic strength. The findings demonstrate that [Hg(II)] and pH are the crucial factors that substantially affect the reaction rate. INH interacts with [Ru(CN)6]4– in a 1 : 1 ratio. At low concentrations, the reaction is first-order dependent on , whereas at higher concentrations, it follows fractional order kinetics. In the analyzed ranges of [INH], the reaction reveals first-order kinetics. The linear decline in reaction rate with the addition of electrolytes signifies a negative salt effect. With rising [Hg(II)], complicated behavior in the reaction rate was noticed. The calculated value of activation parameters viz. entropy of activation, enthalpy of activation, and energy of activation are –279.89, 276.35, and 278.99 kJ M–1, respectively. A relevant mechanistic scheme that is consistent with the experimental data and is endorsed by activation parameters has been proposed. [ABSTRACT FROM AUTHOR] |
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