5. Considering that KpCT)=(Pa AP )ea , what is the equilibrium constant for the

Question

5. Considering that KpCT)=(Pa AP )ea , what is the equilibrium constant for the following reaction at 500 K and a total pressure of 2 bar assuming that there is 1 mole of NO2 present in the system initially. The ratio of the partial pressures at equilibrium of NO2 to NO is: No, = 2.20. (hint: you'll probably want to calculate the mole fraction of everything 1st and use that to get the partial pressures for each species) in Zw%,,-2.20. (hint yo norte partial pressures at equilibrenom ANS : Kp: 0.05630-1543

Explanation / Answer

Keq=[NO]^2[O2]/[No2]^2

Then for gases

Keq=P^2NO.Po2/P^NO2 Then Pno/Pno2=1/2.20

Putting the value in above equation and get the answer

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