Posted by Linda on Wednesday, May 2, 2007 at 5:49pm.
Well I almost understand this question but still got stuck, I will show you the question and my answer so I need someone to tell me if I did it correctly or not and how I should fix it.
at 55degrees the K for the reaction: 2NO2(g)<=>N2O4 is 1.15
calc the concentration of N2O4 present in equilibrium with 0.50 mole of NO2
I first used the ICE chart then calculated
1.15 = x/(0.5-2x)^2
O.5-2x~ ).5
1.15 = x/(0.5)^2
1.15(0.25) = x
x= 0.2875
2(0.2875) - 0.575
Therefore N2O4 = 0.575M?
I dont agree that you can assume .5-2x is approximately .5. Your final answer shows that it is not.
1.15 = x/(0.5-2x)^2
(0.5-2x)^2= x/1.15
.25 -2x +4x^2= .696x
put the terms together, and use the quadratic equation for x.
then would my answer look like this
0.25-2.696x + 4x^2 = 0
and I would also like to understand how did you get 0.696?
I dont know how I got .696 . It should have been 1/1.15=.869
Now that you have the quadratic,
0.25-2.896x + 4x^2 = 0
Use the quadratic equation
x= (2.896 +- sqrt (8.23-4) )/8
x= .618
or x=.104
Now obviously, the first is impossible (why?), so the concentration the product is .104, and the concentration of the reactant is .5-.208
check my calc work
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