For the reaction I_2 + 2S_2O_3^{2-} rightarro | vedclass

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(C) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: Rate $= -\frac{1}{a}\frac{d[A]}{dt} = -\frac{1}{b}\frac{d[B

Vedclass · Accepted Answer

$-\frac{d[I_2]}{dt} = \frac{d[S_4O_6^{2-}]}{dt}$

Vedclass · Answer

(C) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: Rate $= -\frac{1}{a}\frac{d[A]}{dt} = -\frac{1}{b}\frac{d[B]}{dt} = \frac{1}{c}\frac{d[C]}{dt} = \frac{1}{d}\frac{d[D]}{dt}$. For the given reaction $I_2 + 2S_2O_3^{2-} \rightarrow 2I^{-} + S_4O_6^{2-}$,the rate expression is: Rate $= -\frac{d[I_2]}{dt} = -\frac{1}{2}\frac{d[S_2O_3^{2-}]}{dt} = \frac{1}{2}\frac{d[I^{-}]}{dt} = \frac{d[S_4O_6^{2-}]}{dt}$. Comparing this with the given options,the expression $-\frac{d[I_2]}{dt} = \frac{d[S_4O_6^{2-}]}{dt}$ is correct.

For the reaction $I_2 + 2S_2O_3^{2-} \rightarrow 2I^{-} + S_4O_6^{2-}$,which of the following expressions correctly represents the rate of reaction?

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