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  • Half-life for a first order reaction is 693 s. Calculate the time required for 90% completion of this reaction.        

Half-life for a first order reaction is 693 s. Calculate the time required for 90% completion of this reaction.

 

 

 

 
 
 
 
 

Answers (1)

1st order reaction

t_{\frac{1}{2}}=\frac{0.693}{k}

t_{\frac{1}{2}}=693s

k=\frac{0.693}{t_{\frac{1}{2}}}=\frac{0.693}{693}=\frac{1}{1000}=0.001s^{-1}

t_{90%} =?

k=\frac{2.303}{t}\log \frac{\left [ R \right ]_{o}}{\left [ R \right ]}

t_{90}=\frac{2.303}{k}\log \frac{\left [ R \right ]_{0}}{\left [ R \right ]_{0}-0.90\left [ R \right ]_{0}}

t_{90}=\frac{2.303}{0.001}\log 10

t_{90}=\frac{2.303}{0.001}\times 1

t_{90}=2303 s

Posted by

Sumit Saini

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