Question

Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation:

Answer 1

Answer: The initial rate of appearance of chlorite ion under those same conditions is $1.15\times 10^{-1}M/s$  

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

$2ClO_2(aq)+2OH^-(aq)\rightarrow ClO_2^{-}(aq)+ClO_3^{-}(aq)+H_2O(l)$

 The rate in terms of reactants is given as negative as the concentration of reactants is decreasing with time whereas the rate in terms of products is given as positive as the concentration of products is increasing with time.

Rate in terms of disappearance of =  

Rate in terms of appearance of =  

The rate of disappearance of chlorine dioxide = $2.30\times 10^{-1} M/s$

$\frac{d[ClO_2]}{2dt}=\frac{d[ClO_2^{-}]}{dt}$  

$\frac{2.30\times 10^{-1}}{2}=\frac{d[ClO_2^{-}]}{dt}$  

$\frac{d[ClO_2^{-}]}{dt}=1.15\times 10^{-1}M/s$  

The initial rate of appearance of chlorite ion under those same conditions is $1.15\times 10^{-1}M/s$