Question

The rate constant of a second order reaction is ${10}^{-2}lit.mol{e}^{-1}.se{c}^{-1}$. The rate constant when expressed as $cc.molecul{e}^{-1}.mi{n}^{-1}$ is:

• A. $9.96\times {10}^{-22}$
• B. $9.96\times {10}^{-23}$
• C. $9.96\times {10}^{-21}$
• D. $9.96\times {10}^{-24}$

Answer 1

The correct option is A $9.96\times {10}^{-22}$

The rate constant of a second order reaction is ${10}^{-2}lit.mol{e}^{-1}.se{c}^{-1}$.
$1L=1000cc$

$1mole=6.023\times {10}^{23}$molecules
$1min=60sec$
Hence, rate constant $={10}^{-2}lit.mol{e}^{-1}se{c}^{-1}\times \frac{1000cc}{1L}\times \frac{1mole}{6.023\times {10}^{23}molecules}\times \frac{60sec}{1min}$
$=9.96\times {10}^{-22}ccmolecul{e}^{-1}mi{n}^{-1}$