for the reaction S2F6 (g) 2SF2(g), the equilibrium concentrations are as follows: [S26]=0.000430M, [SF2]=2.08 M, [F2]=1.32M. the equilibrium constant is
You should be more careful in your posts. Half of the information you list either is a typo or incorrect. My answer is based on assumptions as to what you meant to post.No arrow. Equation is missing F2, I assume. S26 I assume is S2F6 and so on into the evening.
Keq = (SF2)^2(F2)/(S2F6)
Keq = (2.08)^2(1.32)/0.000430
To find the equilibrium constant (Kc) for the given reaction S2F6 (g) ⇌ 2SF2(g), we need to use the equilibrium concentrations of the reactants and products.
The equilibrium constant expression for the given reaction is:
Kc = ([SF2]^2) / ([S2F6])
Now, substitute the given equilibrium concentrations into the expression:
Kc = ([SF2]^2) / ([S2F6])
= (2.08 M)^2 / (0.000430 M)
Calculate the value:
Kc = (4.3264 M^2) / (0.000430 M)
= 10058.14
Therefore, the equilibrium constant (Kc) for the reaction S2F6 (g) ⇌ 2SF2(g) is approximately 10058.14.
To determine the equilibrium constant for the reaction S2F6(g) ⇌ 2SF2(g), we need to use the equilibrium concentrations provided.
The general form of the equilibrium expression for a reaction aA + bB ⇌ cC + dD is:
Kc = [C]^c [D]^d / [A]^a [B]^b
In this case, the balanced equation is S2F6(g) ⇌ 2SF2(g), so we have a = 1 (coefficient of S2F6), b = 0 (no B in the equation), c = 2 (coefficient of SF2), and d = 0 (no D in the equation).
Plugging in the given equilibrium concentrations:
Kc = [(2SF2)^2] / [S2F6]
The concentration of [S2F6] is given as 0.000430 M. The concentration of [SF2] is given as 2.08 M, but since SF2 is squared in the equilibrium expression, we must square this concentration as well:
[SF2]^2 = (2.08)^2
Now we can substitute these values into the equilibrium expression:
Kc = [(2.08)^2] / (0.000430)
Simplifying this expression will give the value of the equilibrium constant.