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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

  • chem -

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

  • chem -

    N2O4 -> 2NO2

    I 1.596 1.008


    C .252 -.504


    E 1.845 .504

  • chem -

    1.596+0.252 = 1.848.

  • chem -

    that would still be 1.85 with 3 sig figs

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