Consider the following balanced chemical equation:

$H_2{O}_2(aq)+3I_{(aq)}^{-}+2H_{(aq)}^{+}{I}_3^{-}(aq)+2H_{2}O(I)$

In the first $24\mathrm{.}9$ seconds of the reaction, the concentration of $I_3-$ increased from $0\mathrm{.}67M$ to $0\mathrm{.}901M.$

What is the average reaction rate over this time interval $($in $mol{L}^{-1}{s}^{-1})?$

Remember: if you want to express an answer in scientific notation, use the letter $"$E$".$ For example $"4\mathrm{.}32$ x ${10}^4$ should be entered as $"4\mathrm{.}32$E$4".$

Answer: