C(g) + 2A(g) ⇌ 3E(s) + 2F(g)
The concentrations of C, A, and F are measured as 0.2 M, 0.2 M, and 0.4 M at equilibrium and at 100 K.
What is the value of the equilibrium constant?
a. 25
b. 20
c.10
d. 15
[F]^2 / ([C] [A]^2)
so 20 right?
right
To determine the value of the equilibrium constant (K) for the given reaction, you need to use the equilibrium concentrations of the reactants and products.
The equilibrium constant expression (Kc) is written as:
Kc = ([E]^3 * [F]^2) / ([C] * [A]^2)
Given the equilibrium concentrations:
[C] = 0.2 M
[A] = 0.2 M
[F] = 0.4 M
Substituting these values into the equilibrium constant expression, we get:
Kc = (0.2^3 * 0.4^2) / (0.2 * 0.2^2)
Kc = (0.008 * 0.16) / (0.04 * 0.04)
Kc = 0.00128 / 0.0016
Kc = 0.8
Therefore, the value of the equilibrium constant (K) for the given reaction is 0.8.
None of the options provided (a, b, c, or d) match the calculated value.