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JEE Main & Advanced Sample Paper JEE Main - Mock Test - 1

  • question_answer
    Consider the reaction: \[{{N}_{2}}(g)+3{{H}_{2}}(g)\to 2N{{H}_{3}}(g)\]The equality relationship between \[\frac{d[N{{H}_{3}}]}{dt}\] and \[-\frac{d[{{H}_{2}}]}{dt}\]is

    A) \[+\frac{d[N{{H}_{3}}]}{dt}=-\frac{2}{3}\frac{d[{{H}_{2}}]}{dt}\]

    B) \[+\frac{d[N{{H}_{3}}]}{dt}=-\frac{3}{2}\frac{d[{{H}_{2}}]}{dt}\]

    C) \[\frac{d[N{{H}_{3}}]}{dt}=-\frac{d[{{H}_{2}}]}{dt}\]

    D) \[\frac{d[N{{H}_{3}}]}{dt}=-\frac{1}{3}\frac{d[{{H}_{2}}]}{dt}\]

    Correct Answer: A

    Solution :

    If we write rate of reaction in terms of concentration of \[N{{H}_{3}}\] and \[{{H}_{2}}\] then Rate of reaction \[=\frac{1}{2}\frac{d[N{{H}_{3}}]}{dt}=-\frac{1}{3}\frac{d[{{H}_{2}}]}{dt}\] So,  \[\frac{d[N{{H}_{3}}]}{dt}=-\frac{2}{3}\frac{d[{{H}_{2}}]}{dt}\]


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