Question #7bc48
1 Answer
Here's what I got.
Explanation:
Start by calculating the initial concentration of nitrosyl chloride
#["NOCl"] = "0.80 moles"/"2.0 L" = "0.40 mol L"^(-1)#
Now, the balanced chemical equation that describes this equilibrium looks like this
#2"NOCl"_ ((g)) rightleftharpoons 2"NO"_ ((g)) + "Cl"_ (2(g))#
As you can see, for every
This means that if you take
#["NO"] = xcolor(white)(.)"mol L"^(-1)# #["Cl"_2] = (1/2 * x) color(white)(.)"mol L"^(-1)# #["NOCl"] = (0.40 - x)color(white)(.)"mol L"^(-1)#
This basically means that in order for the reaction to produce
By definition, the equilibrium constant for this reaction looks like this
#K_c = (["NO"]^2 * ["Cl"_2])/(["NOCl"]^2)#
In your case, you have--I won't add the units here
#1.60 * 10^(-5) = (x^2 * (1/2x))/((0.40 - x)^2)#
#1.60 * 10^(-5) = (1/2x^3)/((0.40 - x)^2)#
This will be equivalent to
#x^3 + 3.2 * 10^(-5) * x^2 + 1.024 * 10^(-5) * x - 0.512 * 10^(-5)= 0#
This cubic equation will produce three solutions, one positive and two negative. Since
#x = 0.017#
This means that, at equilibrium, the reaction vessel will contain
#["NOCl"] = (0.40 - 0.017)color(white)(.)"mol L"^(-1) = "0.38 mol L"^(-1)#
#["NO"] = "0.017 mol L"^(-1)#
#["Cl"_2] = (1/2 * 0.017)color(white)(.)"mol L"^(-1) = "0.0090 mol L"^(-1)#
All the values are rounded to two sig figs.
SIDE NOTE: Notice that you can't use the approximation
#0.40 -x ~~ 0.40#
because, in that case, you would get
#1.60 * 10^(-5) = (1/2x^3)/0.40^2#
Rearrange to solve for
#x = root(3)( (1.60 * 10^(-5) * 0.40)/(1/2))= 0.023#
In order for that approximation to hold, you need to have
#(["NO"])/(["NOCl"]_0) xx 100% < color(red)(5%)#
However, this is not the case because
#(0.023 color(red)(cancel(color(black)("mol L"^(-1)))))/(0.40color(red)(cancel(color(black)("mol L"^(-1))))) xx 100% = 5.75% > color(red)(5%)#
which implies that the approximation is not valid.