A) \[2.5\times {{10}^{-4}}mol\,{{L}^{-1}}{{s}^{-1}}\]
B) \[5.0\times {{10}^{-4}}mol\,{{L}^{-1}}{{s}^{-1}}\]
C) \[2.5\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]
D) \[1.0\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]
Correct Answer: A
Solution :
Key Idea: Write rate law expression for the reaction. \[\therefore \] \[\frac{-d[A]}{dt}=-\frac{1}{2}\frac{d[B]}{dt}=\frac{d[C]}{dt}=\frac{d[D]}{dt}\] Given, \[-\frac{d[A]}{dt}=5\times {{10}^{-4}}mol\,{{L}^{-1}}{{s}^{-1}}\] \[\because \] \[-\frac{d[A]}{dt}=-\frac{1}{2}\frac{d[B]}{dt}\] \[\therefore \] \[-\frac{1}{2}\frac{d[B]}{dt}=5\times {{10}^{-4}}mol\,{{L}^{-1}}{{s}^{-1}}\] \[\therefore \] \[\frac{d[B]}{dt}=\frac{5\times {{10}^{-4}}}{2}=2.5\times {{10}^{-4}}\,mol\,{{L}^{-1}}{{s}^{-1}}\]
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