A reaction is represented by this equation:
2W(
aq
) ⇌ X(
aq
) + 2Y(
aq
)
K
c
= 5 × 10
−4
(a) Write the mathematical expression for the equilibrium constant.
(b) Using concentrations of ≤1
M
, make up two sets of concentrations that describe a mixture of W, X, and Y at
equilibrium.
(a) The mathematical expression for the equilibrium constant (Kc) is given by:
Kc = [X]^1 * [Y]^2 / [W]^2
where [X], [Y], and [W] represent the equilibrium concentrations of X, Y, and W, respectively.
(b) To create two sets of concentrations that describe a mixture at equilibrium, we need to assign random values to the concentrations within the given range (≤ 1 M). Here are two examples:
Set 1:
[W] = 0.1 M
[X] = 0.02 M
[Y] = 0.05 M
Set 2:
[W] = 0.8 M
[X] = 0.1 M
[Y] = 0.3 M
Please note that the actual equilibrium concentrations depend on various factors and experimental conditions and cannot be determined solely based on the given equation and range.
(a) The mathematical expression for the equilibrium constant (Kc) is determined by the concentrations of the reactants and products at equilibrium. In this case, the equation is:
Kc = [X]^1 [Y]^2 / [W]^2
Where [X], [Y], and [W] represent the molar concentrations of X, Y, and W respectively.
(b) To create two sets of concentrations describing a mixture at equilibrium, we need to assign values to the concentrations of X, Y, and W. Let's assume the following:
Set 1:
[W] = 0.02 M
[X] = 0.05 M
[Y] = 0.10 M
Set 2:
[W] = 0.10 M
[X] = 0.08 M
[Y] = 0.16 M
Keep in mind that these values are just examples, and any combination of concentrations that satisfies the equation and lies within the given range (≤ 1 M) can be used.