A) 0.5
B) 1.0
C) 1.5
D) 2.0
Correct Answer: B
Solution :
\[0.12\,M\xrightarrow{10\,h}0.06\,M;{{t}_{50%}}=10\,h\] \[0.12\,M\xrightarrow{15\,h}0.045\,M;{{t}_{62.5%}}=15\,h\] \[0.12\,M\xrightarrow{20\,h}0.03\,M;{{t}_{75%}}=20\,h\] For first order reaction, \[{{t}_{75%}}={{t}_{50%}}\times 2\] Hence, this is a first order reaction. Further on putting the values in first order reaction, the value of k remains constant, hence it is a first order reaction.
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