The equilibrium constant, Kc, for the equilibrium
N2O4(g)←→2NO2(g)
is 4.6×10−3 .
If the equilibrium mixture contains 5.0×10−2M NO2, what is the concentration of N2O4?
Kc = [NO2]^2 / [N2O4]
so [N2O4] = [NO2]^2 / Kc
To solve this problem, we can use the equilibrium expression for the reaction:
Kc = [NO2]^2 / [N2O4]
Given: Kc = 4.6×10^(-3) and [NO2] = 5.0×10^(-2) M
We need to find the concentration of N2O4, denoted by [N2O4].
Let's substitute the given values into the equilibrium expression and solve for [N2O4]:
Kc = [NO2]^2 / [N2O4]
4.6×10^(-3) = (5.0×10^(-2))^2 / [N2O4]
Now let's solve for [N2O4]:
[N2O4] = (5.0×10^(-2))^2 / 4.6×10^(-3)
[N2O4] = 2.5×10^(-4) / 4.6×10^(-3)
To simplify this expression, we divide the numerator and denominator by 2.5×10^(-3):
[N2O4] = (2.5×10^(-4) / 2.5×10^(-3)) / (4.6×10^(-3) / 2.5×10^(-3))
Simplifying further, we get:
[N2O4] = 0.1 / 1.84
Calculating this division, we find:
[N2O4] ≈ 0.054 M
Therefore, the concentration of N2O4 in the equilibrium mixture is approximately 0.054 M.
To find the concentration of N2O4 in the equilibrium mixture, we can use the equilibrium constant (Kc) and the concentration of NO2 given in the question.
The equilibrium constant (Kc) is defined as the ratio of the products' concentrations to the reactants' concentrations, each raised to the power of their respective stoichiometric coefficients.
For the given equilibrium reaction:
N2O4(g) ⇌ 2NO2(g)
The equilibrium constant expression is:
Kc = [NO2]^2 / [N2O4]
We are given that Kc is 4.6×10^−3 and the concentration of NO2 is 5.0×10^−2 M.
Substituting the given values into the equilibrium constant expression:
4.6×10^−3 = (5.0×10^−2)^2 / [N2O4]
Now, we can rearrange the equation and solve for [N2O4]:
[N2O4] = (5.0×10^−2)^2 / 4.6×10^−3
[N2O4] = 2.38 M
Therefore, the concentration of N2O4 in the equilibrium mixture is 2.38 M.
........N2O4 ==> 2NO2
E.......x.........5E-2M
Kc = 4.6E-3 = (NO2)^2/(N2O4)
Substitute and solve for N2O4.