For the second-order reaction below,the initial concentration of A is 1.34 M.If k = 7.61 × 10?⁴ M¹s?¹,what is the concentration of A after 18.3 minutes? $2 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}$

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The Answer of For the second-order reaction below,the initial concentration of A is 1.34 M.If k = 7.61 × 10?⁴ M¹s?¹,what is the concentration of A after 18.3 minutes? $2 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}$

For the Second-Order Reaction Below,the Initial Concentration of a Is 2 A→B rate =k[ A]22 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}2 A→B rate =k[ A]2

For the Second-Order Reaction Below,the Initial Concentration of a Is $2 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}$