Question

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

Answer 1

If you had typed in your work I could have found the error.

Answer 2

N2O4 -> 2NO2

I 1.596 1.008


C .252 -.504


E 1.845 .504

Answer 3

1.596+0.252 = 1.848.

Answer 4

that would still be 1.85 with 3 sig figs