[THISMOMENTISFATE]

i am so confused, how do i solve this?

all i know so far is that i have to figure out what numbers to put in:

[2NO2 NUMBER]^2
-------------------
[N204 NUMBER]

But im not sure how to find the number for each in this kind of probs. i dont mind solving it myself, can someone help me get started?

Dinitrogentetraoxide partially decomposes according to the following equilibrium:

N2O4 (g) <-> 2NO2 (g)

A 1.00-L flask is charged with 0.400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol ofN2O4
remains. Keq for this reaction is __________.

A) 2.2 x 10-4 B) 13 C) 0.22 D) 0.87 E) 0.022

[Borek]

Use stoichiometry of the reaction to calculate final concentrations.

[THISMOMENTISFATE]

. sorry this is my first time doing this kind of problem and im really lost.

[Borek]

There is nothing complicated here.

Initially there was 0.0400 moles of N₂O₄. Finally there was 0.0055 moles. How many moles decomposed? How many moles of NO₂ were produced?

This is very, very simple stoichiometry, nothing fancy.