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  • The rate constant of a reaction is <img alt="1.25 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}" src="https://entrancecorner.oncodecogs.com/gif.latex?1.25%20%5Ctimes%2010%5E%7B-4%7

The rate constant of a reaction is 1.25 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}. If the initial concentration of the reactant is 2 \mathrm{~mol} \mathrm{~L}^{-1}, the total time (in seconds) required for 75 \% conversion is:
 

Option: 1

\mathrm{1999 \: to\: 2001}
 


Option: 2

\mathrm{5999 \: to\: 6001}


Option: 3

\mathrm{11999 \: to\: 12001}


Option: 4

\mathrm{15999 \: to\: 16001}


Answers (1)

best_answer

\mathrm{ \because K=1.25 \times 10^{-4} \mathrm{~mol}^{-1} \mathrm{~s}^{-1} }

By unit, zero th order reaction.

\mathrm{ [R]=[R]_0-k t }

For \mathrm{ 75 \% } conversion, \mathrm{ [R]=\frac{[R]_0}{4} }

\mathrm{ t_{75 \%}=\frac{3\left[R_0\right]}{4 \mathrm{~K}} }

\mathrm{ t_{75 \%}=\frac{3 \times 2}{4 \times 1.25 \times 10^{-4}} }

\mathrm{ t_{75 \%}=6 \times 2000=12000 \text { seconds } }

Hence option 3 is correct.



 

Posted by

Suraj Bhandari

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