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For reaction $C+D\rightarrow A+B$,the rate expression is rate=$k[C]^{1/2}[D]^{1/2}$ starting with initial concentration of 4M of C and D each,what is time taken for concentration of A to become 0.25M.Given :$k=2.303\times 10^{-2}sec^{-1}$

$(a)\;60sec\qquad(b)\;30sec\qquad(c)\;120sec\qquad(d)\;None$

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Answer: 120 s
$t=\large\frac{1}{k}$$ln\large\frac{[A_o]}{[A_t]}$
Taking $\log_{10}$, $t=\large\frac{2.303}{2.303\times 10^{-2}}$$\log\large\frac{4}{0.25}$
$\Rightarrow t=100\times 4\times 0.3 = 120\;s$
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