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JEE Main & Advanced JEE Main Paper (Held on 10-4-2019 Afternoon)

  • question_answer
    For the reaction, \[2S{{O}_{2}}(g)+{{O}_{2}}(g)\rightleftharpoons 2S{{O}_{3}}(g),\]\[\Delta H=-57.2kJ\,mo{{l}^{-1}}\] and \[{{K}_{c}}=1.7\times {{10}^{16}}.\] Which of the following statement is INCORRECT?             [JEE Main 10-4-2019 Afternoon]

    A) The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required.

    B) The equilibrium will shift in forward direction as the pressure increase.

    C) The equilibrium constant decreases as the temperature increases.

    D) The addition of inert gas at constant volume will not affect the equilibrium constant.

    Correct Answer: A

    Solution :

    In option [b]\[-\Delta {{n}_{g}}\] is -ve therfore increase in pressure will bring reaction in forward direction. In option [c]- as the reaction is exothermic therefore increase in temperature will decrease the equilibrium constant. In option [d]- Equillibrium constant changes only with temperature. Hence, option [b], [c] and [d] are correct therefore option [a] is incorrect choice.


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