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JEE Main & Advanced JEE Main Paper (Held On 16 April 2018)

  • question_answer
    The gas phase reaction \[2N{{O}_{2}}(g)\to {{N}_{2}}{{O}_{4}}(g)\]is an exothermic reaction. The decomposition of\[{{N}_{2}}{{O}_{4}},\] in equilibrium mixture of \[N{{O}_{2}}(g)\]and \[{{N}_{2}}{{O}_{4}}(g),\]can be increased by: [JEE Main 16-4-2018]

    A)  A increasing the pressure

    B)  addition of an inert gas at constant pressure

    C)  lowering the temperature

    D)  addition of an inert gas at constant volume

    Correct Answer: B

    Solution :

     reaction at equilibirium (1) according to Le chatelier's principle- Increasing the pressure on a gas reaction shifts the position of equilibirium towards the side with fewer molecules. So, It will move in backward direction which leads to formation of\[{{N}_{2}}{{O}_{4}}\]from\[N{{O}_{2}}.\]So option (1) is correct. (2)addition of an inert gas at constant pressure will increases volume and equilibirium shifts towards more number of molecules. (3) Decomposition of will be endothermic, so reaction will move in forward reaction when temperature is increased. So, It is incorrect. It will not effect reaction (volume is constant)


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