An equilibrium mixture of the following reaction was found to have [SO3] = 0.391 M and [O2] = 0.125 M at 600 °C. What is the concentration of SO2?
2 SO2 (g) + O2 (g) ====== 2 SO3 (g)
Keq = 4.34 at 600 °C
Kc = (SO3)^2/(SO2)^2(O2)
You K, SO3 and O2. Solve for the only unknown there, SO2.
Jabs
To find the concentration of SO2, we can use the equilibrium expression and the given concentrations of SO3 and O2.
The equilibrium expression for the reaction is:
Keq = [SO3]^2 / ([SO2]^2 * [O2])
Given:
[SO3] = 0.391 M
[O2] = 0.125 M
Keq = 4.34
Now we can rearrange the equilibrium expression to solve for [SO2]:
[SO2]^2 = [SO3]^2 / (Keq * [O2])
[SO2]^2 = (0.391)^2 / (4.34 * 0.125)
[SO2]^2 = 0.014236 / 0.5425
[SO2]^2 = 0.026249
Taking the square root of both sides:
[SO2] = √0.026249
[SO2] = 0.162 M
Therefore, the concentration of SO2 is 0.162 M.
To find the concentration of SO2, we need to use the equilibrium constant (Keq) expression and the concentrations of the other substances.
The balanced equation for the reaction is:
2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g)
The equilibrium constant expression for this reaction is:
Keq = [SO3]^2 / ([SO2]^2 * [O2])
We are given the equilibrium concentrations of [SO3] = 0.391 M and [O2] = 0.125 M. We need to rearrange the equilibrium constant expression to solve for [SO2].
Letting x be the concentration of SO2, the equilibrium constant expression becomes:
4.34 = (0.391)^2 / (x^2 * 0.125)
Now we can solve for x:
4.34 = 0.391^2 / (x^2 * 0.125)
4.34 * x^2 * 0.125 = 0.391^2
x^2 = (0.391^2) / (4.34 * 0.125)
x = √[(0.391^2) / (4.34 * 0.125)]
Calculating this expression will give us the concentration of SO2.