JEE Main & Advanced Sample Paper JEE Main - Mock Test - 18

  • question_answer
    In the case of a first order reaction, the time required for \[93.75%\] of reaction to take place is x times that required for half of the reaction. Find the value of x.

    A) 2                      

    B)        3                     

    C) 4          

    D)        5

    Correct Answer: C

    Solution :

        [c] \[{{t}_{1/2}}=\frac{0.0693}{{{k}_{1}}}\] Also,  \[{{t}_{93.75}}=\frac{2.303}{{{k}_{1}}}\log \frac{100}{100-93.75}\] \[=\frac{2.303}{{{k}_{1}}}\log \frac{100}{6.25}=\frac{4\times 2.303\times \log 2}{{{k}_{1}}}=\frac{4\times 0.693}{{{k}_{1}}}=4{{t}_{1/2}}\]       


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