Consider the reaction:
SO2Cl2(g)⇌SO2(g)+Cl2(g)
A solution is made containing initial [SO2Cl2]= 0.022M . At equilibrium, [Cl2]= 1.7×10−2M
Calculate the value of the equilibrium constant.
..........SO2Cl2 ==> SO2 + Cl2
I.........0.022......0......0
C.........-x.........x......x
E.......0.022-x......x......x
The problems tell you that (Cl2) = x = 1.7E-2.
Substitute into Kc expression and calculate Kc
To calculate the value of the equilibrium constant (K), you need to use the concentrations of the reactants and products at equilibrium.
First, let's write the expression for the equilibrium constant (K) for the given reaction:
K = [SO2(g)] * [Cl2(g)] / [SO2Cl2(g)]
Now, we are given the concentrations of [Cl2] and [SO2Cl2] at equilibrium. However, we need the concentration of [SO2(g)] to calculate the value of K.
To determine the concentration of [SO2(g)] at equilibrium, we can use the stoichiometry of the balanced equation. According to the balanced equation:
1 mol of SO2Cl2 produces 1 mol of SO2
Since the initial concentration of [SO2Cl2] is given as 0.022 M and the concentration of [Cl2] at equilibrium is 1.7×10^−2 M, we can assume that at equilibrium, an equal amount of SO2 is formed.
So, the concentration of [SO2(g)] at equilibrium is also 1.7×10^−2 M.
Now we have the values to calculate the equilibrium constant:
K = [SO2(g)] * [Cl2(g)] / [SO2Cl2(g)]
Substituting the values:
K = (1.7×10^−2) * (1.7×10^−2) / (0.022)
K = 0.000289 / 0.022
K ≈ 0.0132 (rounded to four decimal places)
Therefore, the value of the equilibrium constant (K) for the given reaction is approximately 0.0132.
The equilibrium constant (K) for the reaction is calculated using the concentrations of the reactants and products at equilibrium.
Given:
Initial concentration of SO2Cl2 ([SO2Cl2]initial) = 0.022 M
Concentration of Cl2 ([Cl2]equilibrium) = 1.7 × 10^(-2) M
Using the stoichiometry of the reaction, we can determine the concentrations of the other species at equilibrium:
After the reaction has reached equilibrium, let [SO2Cl2]equilibrium = x M and [SO2]equilibrium = [Cl2]equilibrium = 1.7 × 10^(-2) M.
The equilibrium expression for the reaction is:
K = ([SO2]equilibrium * [Cl2]equilibrium) / [SO2Cl2]equilibrium
Substituting the given values:
K = (1.7 × 10^(-2) M * 1.7 × 10^(-2) M) / (x M)
We can now solve for x:
0.022 M = x M
Therefore, x = 0.022 M.
Now, substituting x back into the equation for K:
K = (1.7 × 10^(-2) M * 1.7 × 10^(-2) M) / (0.022 M)
K = 0.1225 M^2 / 0.022 M
K = 5.568
So, the value of the equilibrium constant (K) for the given reaction is 5.568.