The following reaction:
2SO3 (g) ! 2SO2 (g) + O2 (g) has an equilibrium constant equal to 0.23 M. If the following concentrations are present:
[SO2] =0.480 M, [O2] = 0.561 M, [SO3] = 0.220 M, is the reaction at equilibrium? If not, which way must it shift to reach equilibrium?
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Find the reaction quotient or Q.
Q = (SO2)^2 x (O2)/(SO3)^2
Q = (0.480)^2(0.561)/(0.220)^2
Q = 2.67
Compare this to K = 0.23 in the problem.
Q is to high meaning SO2 and O2 are too high and SO3 is too low; therefore, it much shift to the left to reach equilibrium. That way SO2 and O2 are lowered and SO3 is raised.
To determine whether the reaction is at equilibrium or not, we need to compare the given concentrations of the reactants and products with the equilibrium constant (K).
The equilibrium constant (K) is calculated by taking the ratio of the product concentrations raised to their respective stoichiometric coefficients divided by the reactant concentrations raised to their respective stoichiometric coefficients.
The given reaction is:
2SO3 (g) → 2SO2 (g) + O2 (g)
The equilibrium constant expression for this reaction can be written as:
K = [SO2]^2 * [O2] / [SO3]^2
Now let's substitute the given concentrations into the equilibrium constant expression:
K = (0.480)^2 * (0.561) / (0.220)^2
K = 0.230
Comparing the calculated equilibrium constant (K) with the given equilibrium constant (0.23 M), we can conclude that the reaction is indeed at equilibrium.
Therefore, the reaction is already at equilibrium, and no shift is required to reach equilibrium.
To determine if the reaction is at equilibrium, we need to compare the given concentrations with the equilibrium constant (Kc) of 0.23 M.
The equilibrium constant expression for the given reaction is:
Kc = [SO2]^2 * [O2] / [SO3]^2
Let's substitute the given concentrations into the equilibrium constant expression:
Kc = (0.480 M)^2 * (0.561 M) / (0.220 M)^2
Kc = 0.1104 M
Since the calculated equilibrium constant (0.1104 M) is not equal to the given equilibrium constant (0.23 M), we can conclude that the reaction is not at equilibrium.
To determine which way the reaction must shift to reach equilibrium, we can compare the calculated Kc value with the given equilibrium constant:
0.1104 M < 0.23 M
Since the calculated Kc value is lower than the given equilibrium constant, the reaction must shift in the forward direction (to the right) to reach equilibrium. This means that more products (SO2 and O2) need to be formed, and the concentration of reactant (SO3) needs to decrease.
In summary, the reaction is not at equilibrium, and it must shift to the right (forward direction) to reach equilibrium.