For the first-order reaction below,the initial concentration of A is 0.240 M.If the concentration of A decreases to 0.0800 M after 21.8 hours,what is the half-life of the reaction? $ \mathrm{A} \rightarrow \mathrm{B} $$ \quad$$ \quad$$ \quad$$ \quad$$ \quad$rate $ =k[\mathrm{~A}] $

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The Answer of For the first-order reaction below,the initial concentration of A is 0.240 M.If the concentration of A decreases to 0.0800 M after 21.8 hours,what is the half-life of the reaction? $ \mathrm{A} \rightarrow \mathrm{B} $$ \quad$$ \quad$$ \quad$$ \quad$$ \quad$rate $ =k[\mathrm{~A}] $

For the First-Order Reaction Below,the Initial Concentration of a Is A→B \mathrm{A} \rightarrow \mathrm{B} A→B

For the First-Order Reaction Below,the Initial Concentration of a Is $\mathrm{A} \rightarrow \mathrm{B}$