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JIPMER Jipmer Medical Solved Paper-2001

  • question_answer
    The rate of a first order reaction is\[0.693\times {{10}^{-2}}\,mol\,{{L}^{-1}}\,{{\min }^{-1}}\] and the initial concentration of the reactants is 1 M, \[{{t}_{1/2}}\] is equal to:

    A)  6.92 minute

    B)  100 minutes

    C)  \[0.693\times {{10}^{-3}}\]minute           

    D)  \[0.693\times {{10}^{-2}}\]minute

    Correct Answer: B

    Solution :

    For 1st order reaction, \[\text{rate}=K\times [A]\] \[\therefore \]  \[0.693\times {{10}^{-2}}=K\times 1\] or            \[K=0.693\times {{10}^{-2}}{{\min }^{-1}}\] We know that, \[{{t}_{1/2}}=\frac{0.693}{K}=\frac{0.693}{0.693\times {{10}^{-2}}}\]        = 100 minute


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