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A flask containing pure NO2 was heated to 1250K, a temperature at which the Kpvalue for the...

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Chemistry

A flask containing pure NO2 was heated to 1250K, atemperature at which the Kpvaluefor the decomposition of NO2 is 177.

2 NO2(g) <---------> 2 NO(g) +O2(g)

Starting with pure NO2 , the flask is heated and hepartial pressure of O2 at equlibrium is 0.133 am. Calculate thepartial pressures of NO and NO2 at equlibrium and thetotal pressure in the flask at equlibrium.

PNO ____________________atm

PNO2____________________atm

Ptotal____________________atm

Answer & Explanation Solved by verified expert
3.8 Ratings (598 Votes)

                                 2 NO2(g) <---------> 2 NO(g) + O2(g)

Equb pressure             2p                         2p            p

Equilibrium constant , Kp = (p2NO x pO2 ) / p2NO2

Given equilibrium partial pressure of O2 is 0.133 atm

So Equilibrium partial pressure of NO = 2p = 2x0.133 = 0.266 atm

Equilibrium partial pressure of NO2 = 2p = 2x0.133 = 0.266 atm

Total pressure of the reaction mixture = partial pressure of NO2 + partial pressure of NO + partial pressure of O2

= 0.266+0.266+0.133

= 0.665 atm       

                 
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