At a particular temperature, 13.7 mol of SO3 is placed into a 3.9-L rigid container, and the SO3 dissociates by the reaction given below.
2 SO3(g) 2 SO2(g) + O2(g)
At equilibrium, 3.8 mol of SO2 is present. Calculate K for this reaction.
13.7mol/3.9L = about 3.5
3.8/3.9 = about0.97
You need to do these more accurately.
........SO3 ==> 2SO2 + O2
I.......3.5.......0......0
C.......-2x.....2x.......x
E......3.5-2x...2x........x
The problem tells you that at equilibrium (SO2) = 2x = 3.8/3.9 = 0.974M
Knowing x, you can calculate SO2m O2, and SO3, then substitute into the Kc expression and solve for Kc.
it says my answer is still wrong. I got 0.017683 but it says the right answer is 0.071777081878092.
To calculate the equilibrium constant, K, for this reaction, we need to use the concentrations of the species at equilibrium.
Given:
Initial number of moles of SO3 = 13.7 mol
Moles of SO2 at equilibrium = 3.8 mol
Total volume of the container = 3.9 L
At equilibrium, we can assume that the volume of gases is negligible compared to the volume of the container. Therefore, we can directly use the concentration of SO2 at equilibrium.
To find the concentration of SO2, we use the formula:
(concentration) = (moles) / (volume)
The concentration of SO2 at equilibrium = (3.8 mol) / (3.9 L)
= 0.9744 M
Since the stoichiometric coefficient for SO2 in the balanced chemical equation is 2, the concentration of SO3 at equilibrium can be calculated as:
(concentration of SO3 at equilibrium) = (concentration of SO2 at equilibrium) / 2
= 0.9744 M / 2
= 0.4872 M
The concentration of O2 at equilibrium can also be calculated:
(concentration of O2 at equilibrium) = (concentration of SO2 at equilibrium) / 2
= 0.9744 M / 2
= 0.4872 M
Now, we can plug in the equilibrium concentrations into the equilibrium expression and solve for K:
K = [(concentration of SO2)^2 (concentration of O2)] / (concentration of SO3)^2
= [(0.9744 M)^2 * 0.4872 M] / (0.4872 M)^2
= 0.9717
Therefore, the equilibrium constant, K, for this reaction at the given temperature is 0.9717.
To calculate the equilibrium constant (K) for this reaction, we need to use the concentrations (or partial pressures, if dealing with gases) at equilibrium. In this case, we are provided with the number of moles of SO2 at equilibrium, which we can use to find the concentration.
Step 1: Calculate the concentration of SO2:
Since we know the volume of the rigid container is 3.9 L, we can use this information to find the concentration of SO2.
Concentration of SO2 (in M) = Mol of SO2 / Volume of Container (in L)
Concentration of SO2 = 3.8 mol / 3.9 L
Step 2: Calculate the concentration of SO3 at equilibrium:
Since we are given the initial moles of SO3 (13.7 mol) and the balanced equation, we can determine the change in the number of moles of SO3.
From the balanced equation, we can see that for every 2 moles of SO3, the reaction produces 2 moles of SO2.
So, the change in the number of moles of SO3 = initial moles - moles of SO2
Change in moles of SO3 = 13.7 mol - (3.8 mol / 2)
Step 3: Calculate the equilibrium concentration of SO3:
Equilibrium concentration of SO3 = initial concentration - change in concentration
Equilibrium concentration of SO3 = (13.7 mol / 3.9 L) - ((3.8 mol / 2) / 3.9 L)
Step 4: Substitute the concentrations into the equilibrium expression:
K = [SO2]^2 x [O2] / [SO3]^2
K = (3.8 mol / 3.9 L)^2 x [O2] / ((13.7 mol / 3.9 L) - ((3.8 mol / 2) / 3.9 L))^2
Step 5: Solve for K:
Substitute the values of [SO2], [SO3], and solve for K:
K = (3.8^2 x [O2]) / (((13.7 - (3.8 / 2)) / 3.9)^2)
Note: To find the value of K, you would need the concentration of O2 at equilibrium. If the concentration of O2 is not given, you cannot calculate the equilibrium constant (K) without additional information.