• Calculate the equilibrium concentration of all the species in a flask initially containing only 3.00 atm of NO2.
2NO2 (g) ⇌ N2O4 (g) Kp = 9.3 x 10-7
Kp = p(N2O4)/p(NO2)^2
9.3*10^-7 = x / (3.00-2x)^2
Since Kp is small, x will be small and can be ignored as compared to 3.00
So, the above expression becomes:
9.3*10^-7 = x / (3.00)^2
x = 8.4*10^-6 atm
So,
At equilibrium:
p(N2O4) = 8.4*10^-6 atm
p(NO2) = 3.00 atm
Answer:
p(N2O4) = 8.4*10^-6 atm
p(NO2) = 3.00 atm
• Calculate the equilibrium concentration of all the species in a flask initially containing only 3.00...
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