1. Tardigrade
  2. Question
  3. Chemistry
  4. An equilibrium mixture of the reaction 2NO(g)+O2(g)2NO2(g) contains 0.12 moles of NO2 , 0.08 moles of NO and 0.64 moles of 02 in a 4 litre flask at constant temperature. The value of KC this temperature is:

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Q. 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:

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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 $