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 0.750 L 25oC What is the composition of the gaseous mixture when equilibrium is reestablished in the system consisting of the two flasks?

Question

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 <change to>  2.25 L and 25C
0.0580 mol NO2
0.750 L
25oC
What is the composition of the gaseous mixture when equilibrium is reestablished in 
the system consisting of the two flasks?

aaronq · Answer

Can you re-write the question?  it's all over the place

anonymous · Answer

thats what it said in the book.. pretty vague right?

anonymous · Answer

http://www.elcamino.edu/faculty/pdoucette/Chapter-15-problems.pdf page/question no. 3

goformit100 · Answer

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aaronq · Answer

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).