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The decomposition of hydrogen bromide into hydrogen and iodine is second order reaction.The reaction rate constant is $K=0.08Lmol^{-1}s^{-1}$.How long it take an initial concentration of 0.04M to decrease to half this concentration?

$\begin{array}{1 1}(a)\;300sec&(b)\;315sec\\(c)\;212.5sec&(d)\;312.5sec\end{array}$

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$2HBr\rightarrow H_2+Br_2$
At $t=0$ $2HBr\Rightarrow a$
At $t=t$ $2HBr\Rightarrow a-x,H_2\Rightarrow x/2,Br_2\Rightarrow x/2$
Rate $=\large\frac{dx}{2dt}$$=K(a-x)^2$
$K'$=rate constant=0.08$Lmol^{-1}s^{-1}$
$t_{1/2}=\large\frac{1}{0.08\times 0.04}$
Hence (d) is the correct answer.
answered Dec 18, 2013 by sreemathi.v

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