We're asked to find the equilibrium concentrations of
The equilibrium constant expression is given by
$K_c = (["NO"_2]^2)/(["N"_2"O"_4]) = ul(0.36)" "$ $(2000color(white)(l)""^"o""C")$
We'll do our I.C.E. chart in the form of bullet points, for fun. Then, our initial concentrations are
INITIAL
According to the coefficients of the reaction, the amount by which
CHANGE
And so the final concentrations are
FINAL
Plugging these into the equilibrium constant expression gives us
$K_c = ((1-2x)^2)/(x) = ul(0.36)" "$ $(2000color(white)(l)""^"o""C"$ , excluding units$)$
Now we solve for
$(4x^2 - 4x + 1)/x = 0.36$
$4x^2 - 4x + 1 = 0.36x$
$4x^2 - 4.36x + 1 = 0$
Use the quadratic equation:
$x = (4.36+-sqrt((4.36)^2 - 4(4)(1)))/(8) = 0.328color(white)(l)"or"color(white)(l)0.762$
If we plug the larger solution in for
$color(red)("final N"_2"O"_4) = x = color(red)(ulbar(|stackrel(" ")(" "0.33color(white)(l)M" ")|)$
$color(blue)("final NO"_2) = 1-2x = 1-2(0.328) = color(blue)(ulbar(|stackrel(" ")(" "0.34color(white)(l)M" ")|)$ each rounded to
$2$ .