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VIT Engineering VIT Engineering Solved Paper-2007

  • question_answer
    Given the equilibrium system : \[N{{H}_{4}}Cl(s)\xrightarrow{{}}NH_{4}^{+}(aq)+C{{l}^{-}}(aq)\] \[(\Delta H=+3.5kcal/mol.)\] What change will shift the equilibrium to the right?

    A)  Decreasing the temperature                      

    B)  Increasing the temperature                      

    C)  Dissolving  \[NaCl\]   crystals   in   the equilibrium mixture

    D)  Dissolving \[N{{H}_{4}}N{{O}_{3}}\] crystals in the equilibrium mixture

    Correct Answer: B

    Solution :

     \[N{{H}_{4}}Cl(s)\xrightarrow{{}}NH_{4}^{+}(aq)+C{{l}^{-}}(aq)\] \[\Delta H=+3.5kcal/mol\] This is the endothermic reaction hence, increasing the temperature will shift the equilibrium to the right.


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