JEE Main & Advanced Chemistry Chemical Kinetics Question Bank Rate of a reaction

  • question_answer In a catalytic conversion of \[{{N}_{2}}\] to \[N{{H}_{3}}\] by Haber's process, the rate of reaction was expressed as change in the concentration of ammonia per time is \[40\times {{10}^{-3}}\,mol\,litr{{e}^{-1}}{{s}^{-1}}\]. If there are no side reaction, the rate of the reaction as expressed in terms of hydrogen is     (in mol \[litr{{e}^{-1}}{{s}^{-1}}\])

    A)                 \[60\times {{10}^{-3}}\]               

    B)                 \[20\times {{10}^{-3}}\]

    C)                 1.200    

    D)                 \[10.3\times {{10}^{-3}}\]

    Correct Answer: A

    Solution :

               \[\frac{-\,d({{N}_{2}})}{dt}=-\frac{1}{3}\frac{d({{H}_{2}})}{dt}=\frac{1}{2}\frac{d(N{{H}_{3}})}{dt}\]=\[\frac{3}{2}\times 40\times {{10}^{-3}}\]                    \[=60\times {{10}^{-3}}.\]


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