At a particular temperature, 13.4 mol of SO3 is placed into a 3.8-L rigid container, and the SO3 dissociates by the reaction given below.
2 SO3(g) <-> 2 SO2(g) + O2(g)
At equilibrium, 3.6 mol of SO2 is present. Calculate K for this reaction.
I assume you want Kc and not Kp.
13.4 mol/3.8 = approx 3 but that's just an estimate. You can recalculate and use a more accurate number.
........2SO3 ==> 2SO2 + O2
I.......3.........0.....0
C......-2x........2x....x
E......3-2x.......2x....x
You are given mols SO2, convert that to M (which is x), evaluate 2x and 3-2x. plug those numbers into Kc expression and solve for Kc.
Post your work if you get stuck.
To calculate the equilibrium constant, K, for this reaction, we need to use the concentration of the reactants and products at equilibrium.
In the given reaction:
2 SO3(g) <-> 2 SO2(g) + O2(g),
we are provided with the initial amount of SO3 placed in the container, which is 13.4 mol. We are also given the amount of SO2 at equilibrium, which is 3.6 mol.
Since the reaction stoichiometry is 2:2:1 (2 moles of SO3 yielding 2 moles of SO2 and 1 mole of O2), we can say that the amount of O2 at equilibrium is also 3.6 mol.
Now, we need to calculate the equilibrium concentration of the reactants and products. Concentration can be calculated by dividing the amount (in moles) by the total volume (in liters).
The equilibrium concentration of SO3 is calculated as: [SO3] = (amount of SO3 at equilibrium) / (volume of the container)
[SO3] = 13.4 mol / 3.8 L ≈ 3.5263 mol/L
The equilibrium concentration of SO2 is given as 3.6 mol, but since the stoichiometric coefficient is 2, the actual concentration is: [SO2] = 2 * (3.6 mol) / 3.8 L ≈ 1.8947 mol/L
Similarly, the equilibrium concentration of O2 is also: [O2] = 3.6 mol / 3.8 L ≈ 0.9474 mol/L
Now that we have the equilibrium concentrations of the reactants and products, we can write the expression for the equilibrium constant K.
K = ([SO2]^2 * [O2]) / [SO3]^2
Substituting the values:
K = (1.8947^2 * 0.9474) / (3.5263^2)
After performing the calculation, the value of K for this reaction is approximately 0.205.