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 = \[2.0\times {{10}^{-5}}\,\,mol\,{{L}^{-1}}\,{{s}^{-1}}\] \[[A]=Conc.\,\,of\,A=0.01\,M\] \[So\,\,\,\,2.0\times {{10}^{-5}}\,=k\times 0.01\] \[k=\frac{2.0\times {{10}^{-5}}}{0.01}{{s}^{-1}}\] \[=2.0\times {{10}^{-3}}\,{{s}^{-1}}\] 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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