In aqueous solution, thiosulfate ions, $$\(\mathrm{S}_{2} \mathrm{O}_{3}{ }^{2-}\)$$, react with hydrogen ions, as shown in reaction 2. reaction 2 $$\[ \mathrm{S}_{2} \mathrm{O}_{3}{ }^{2-}+2 \mathrm{H}^{+} \rightarrow \mathrm{SO}_{2}+\mathrm{S}+\mathrm{H}_{2} \mathrm{O} \]$$ The rate of reaction is first order with respect to $$\(\left[\mathrm{S}_{2} \mathrm{O}_{3}{ }^{2-}\right]\)$$ and zero order with respect to $$\(\left[\mathrm{H}^{+}\right]\)$$ under certain conditions. The rate constant, $$\(k\)$$, for this reaction is $$\(1.58 \times 10^{-2} \mathrm{~s}^{-1}\)$$. Calculate the half-life, $$\(t_{\frac{1}{2}}\)$$, for reaction 2 . $$\[ t_{\frac{1}{2}}= \]$$ .......................... s

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