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