Dinitrogentetraoxide partially decomposes into nitrogen dioxide. A 1.00-L flask is charged with 0.0400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol of N2O4 remains. Keq for this reaction is .

Keq=0.866

Explanation:

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In this case, the undergone chemical reaction is:

In such a way, since 0.0055 mol of N₂O₄ remains in the flask, one infers that the reacted amount () was:

In addition, the produced amount of NO₂ is:

Finally, considering the flask's volume, the equilibrium constant is then computed as follows:

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po-215 i got it right on the quiz