A flask is charged with 1.596 atm of N2O4(g) and 1.008 atm of NO2(g) at 25°C, and the following equilibrium is achieved.
N2O4(g)-> 2 NO2(g)
After equilibrium is reached, the partial pressure of NO2 is 0.504 atm.
(a) What is the equilibrium partial pressure of N2O4?
for this quetsion i set up an ice box and got 1.85 as my answer but it was wrong.
(c) Calculate the value of Kc for the reaction
4 answers
If you had typed in your work I could have found the error.
N2O4 -> 2NO2
I 1.596 1.008
C .252 -.504
E 1.845 .504
I 1.596 1.008
C .252 -.504
E 1.845 .504
1.596+0.252 = 1.848.
that would still be 1.85 with 3 sig figs
2 answers