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BVP Medical BVP Medical Solved Paper-2001

  • question_answer
     An equilibrium mixture of the reaction \[2NO(g)+{{O}_{2}}(g)2N{{O}_{2}}(g)\]   contains 0.12 moles of \[N{{O}_{2}}\], 0.08 moles of NO and 0.64 moles of 02 in a 4 litre flask at constant temperature. The value of \[{{K}_{C}}\] this temperature is:

    A)  7                                            

    B)  14

    C)  28                                         

    D)  24

    Correct Answer: B

    Solution :

                    \[\underset{At\,equil\,0.08}{\mathop{2NO(g)}}\,+\underset{0.64}{\mathop{{{O}_{2}}(g)}}\,\underset{0.12}{\mathop{2N{{O}_{2}}(g)}}\,,\,\,V=4litre\] \[{{K}_{c}}=\frac{{{[N{{O}_{2}}]}^{2}}}{{{[NO]}^{2}}\,[{{O}_{2}}]}\] \[=\frac{{{\left( \frac{0.12}{4} \right)}^{2}}}{{{\left( \frac{0.08}{4} \right)}^{2}}\times \left( \frac{0.64}{4} \right)}\] \[=\frac{0.12\times 0.12\times 4}{0.08\times 0.08\times 0.64}=14.06\]


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