Question #5fb4f
2 Answers
Explanation:
So, you know that the equilibrium constant,
Right from the start, this tells you that the equilibrium will favor the reactants, since
Since the reaction starts with only the product, you can of course expect that the equilibrium concentration of
You can find the equilibrium concentrations of all the species involved in the reaction by using an ICE table
#"N"_text(2(g]) " "+" " "O"_text(2(g]) " "rightleftharpoons" " color(red)(2)"NO"_text((g])#
By definition, the equilibrium constant for this reaction will be
#K_c = (["NO"]^color(red)(2))/(["N"_2] * ["O"_2]) = ((0.0400-color(red)(2)x)""^color(red)(2))/(x * x)#
#K_c = ((0.0400 - 2x)""^2)/x^2 = 0.050#
Rearrange to get
#3.95x^2 - 0.16x + 0.0016 = 0#
This quadratic equation will produce two positive solutions for
#x_1 = 0.01799" "# and#" "color(red)(cancel(color(black)(x_2 = 0.02252)))#
Therefore, the equilibrium concentrations of the species that took part in the reaction are
#["N"_2] = x = "0.01799 M" = color(green)("0.0180 M")#
#["O"_2] = x = color(green)("0.0180 M")#
#["NO"] = 0.0400 - 2x = 0.0400 - 2 * 0.0180 = color(green)("0.00400 M")#
Explanation:
The forward reaction is:
You should know that the
Therefore, the equilibrium concentrations are:
Replacing the concentrations in the expression of
Solve for
Therefore, the equilibrium concentrations are: