Hi! I need assistance with calculating the equilibrium constant of an overall reaction, yet whatever I try does not work.
The overall reaction is
2Cl2(g) + 10 NO(g) <-> 5N2(g) + 2Cl2O5(g) with Kp=?
I am given:
2Cl2O5(g) <-> 5O2(g) + 2Cl2(g) Kp1 =.095
2NO(g) <-> N2(g) + O2(g) Kp2 =476
So I reversed the first equation given, thus I invert the respective equilibrium constant to get 1/.095; then I noticed that the overall reaction has 10 NO, thus I multiply the second given equation by 5, this requires me taking the equilibrium constant raised to the 5th power, thus I have 4765. Lastly, since I am adding the two equations together, I multiply the two equilibrium constants to get my overall equilibrium constant, which should be (4765)/(.095) however this is incorrect; what is my error?