A) \[3.8\times {{10}^{-2}}s\]
B) \[1.26\times {{10}^{13}}s\]
C) \[2.01\times {{10}^{13}}s\]
D) \[1.097\times {{10}^{3}}\]
Correct Answer: A
Solution :
For a first order reaction, \[t=\frac{2.303}{k}\log \frac{{{[A]}_{0}}}{[A]}\] Here, \[{{A}_{0}}\] = initial concentration A = final concentration Given, \[k=60{{s}^{-1}},[A]={{[A]}_{0}}/10\] Now, \[t=\frac{2.303}{60}\log \frac{{{[A]}_{0}}}{{{[A]}_{0}}/10}\] \[=\frac{2.303}{60}\log 10\] \[=0.038s\] or \[3.8\times {{10}^{-2}}s\]
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