A) \[1.26\times {{10}^{13}}s\]
B) \[2.16\times {{10}^{13}}s\]
C) \[1.26\times {{10}^{-13}}s\]
D) \[2.16\times {{10}^{-13}}s\]
Correct Answer: A
Solution :
For the first order reaction, \[\because \] \[{{t}_{1/2}}=\frac{0.693}{k}\] \[\therefore \] \[=\frac{0.693}{5.5\times {{10}^{-14}}{{s}^{-1}}}\] \[{{t}_{1/2}}=1.26\times {{10}^{13}}s\]
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