Consider the following equilibrium: N2O4(g) ⇌ 2 NO2(g) Kc= 4.61 x 10-3 at 25oC
The N2O4 – NO2 equilibrium mixture in the flask on the left is allowed to expand into the evacuates flask on the right..
0.971 mol N2O4 2.25 L and 25C
0.0580 mol NO2
What is the composition of the gaseous mixture when equilibrium is reestablished in
the system consisting of the two flasks?
Stacey Warren - Expert brainly.com
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Can you re-write the question? it's all over the place
thats what it said in the book.. pretty vague right?
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So, as you decrease the pressure (as you increase the volume) the equilibrium will shift. You need to make an I.C.E. table and calculate the extent the equilibrium will shift (using an equilibrium expression).