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NEET Sample Paper NEET Sample Test Paper-70

  • question_answer
    A mixture of 0.3 mole of \[{{H}_{2}}\] and 0.3 mole of \[{{I}_{2}}\]  is allowed to react in a 10 litre evacuated flask at\[500{}^\circ C\]. The reaction is \[{{H}_{2}}+{{I}_{2}}\rightleftharpoons \,\,2HI\], the K is found to be 64. The amount of unreacted \[{{I}_{2}}\] at equilibrium is

    A) 0.15 mole                    

    B) 0.06 mole

    C) 0.03 mole        

    D) 0.2 mole

    Correct Answer: B

    Solution :

    \[{{K}_{c}}=\frac{{{\left[ HI \right]}^{2}}}{\left[ {{H}_{2}} \right]\left[ {{I}_{2}} \right]}\,\,\,\,\,\,\Rightarrow \,\,\,64=\frac{{{x}^{2}}}{0.03\times 0.03}\] \[{{x}_{2}}=64\times 9\times {{10}^{-}}^{\,4}\] \[x=8\times 3\times {{10}^{-2}}=0.24\] x is the amount of HI at equilibrium amount of \[{{I}_{2}}\]at equilibrium will be                       \[0.30 - 0.24 = 0.06\]


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