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MGIMS WARDHA MGIMS WARDHA Solved Paper-2014

  • question_answer
    For a chemical reaction\[A\to B,\]the rate of the reaction is\[2\times {{10}^{-3}}\]mol\[d{{m}^{-3}}{{s}^{-1}},\]when the initial concentration is 0.05 mol \[d{{m}^{-3}}\]. The rate of the same reaction is\[1.6\times {{10}^{-2}}mol\text{ }d{{m}^{-3}}{{s}^{-1}}\] when the initial concentration is\[0.1\text{ }mol\text{ }d{{m}^{-3}}\]. The order of the reaction is

    A)  2                                            

    B)  0

    C)  3                                            

    D)  1

    Correct Answer: C

    Solution :

                    \[A\xrightarrow{{}}B\] Rate \[=k{{[A]}^{n}}\] \[{{(Rate)}_{1}}=k{{(0.05)}^{n}}=2\times {{10}^{-3}}\] \[{{(Rate)}_{2}}=k{{(0.1)}^{n}}=1.6\times {{10}^{-2}}\] Dividing the Eq. (ii) by Eq. (i) \[\frac{{{(Rate)}_{2}}}{{{(Rate)}_{1}}}=\frac{k{{(0.1)}^{n}}}{k{{(0.05)}^{n}}}=\frac{1.6\times {{10}^{-2}}}{2\times {{10}^{-3}}}\] \[{{(2)}^{n}}=8\]or \[{{(2)}^{n}}={{2}^{3}}\] \[\therefore \]  \[n=3\]


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