A) 220 s
B) 30 s
C) 300 s
D) 347 s
Correct Answer: D
Solution :
For first order reaction, \[A\xrightarrow{{}}B\] Given, that rate \[=k\times [A]\] Rate\[=2.0\times {{10}^{-5}}mol\,{{L}^{-1}}{{s}^{-1}}\] [A] = concentration of A = 0.01 M So \[2.0\times {{10}^{-5}}=k\times 0.01\,K=\frac{2.0\times {{10}^{-5}}}{0.01}{{s}^{-1}}\] \[=2.0\times {{10}^{-3}}{{s}^{-1}}\] For first order reaction, \[{{T}_{1/2}}=\frac{0.693}{k}=\frac{0.693}{2.0\times {{10}^{-3}}}\] \[=346.5=347\,s\]You need to login to perform this action.
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