An equilibrium mixture of the following reaction was found to have = 0.0325 at 1200 degrees C.
What is the concentration of I? I2(g)<->2I (g)
Keq=1.3×10−2 at 1200
0.0325 WHAT molar and WHAT substance?
To find the concentration of I in the equilibrium mixture, we can use the equation for the equilibrium constant (Keq) and the initial concentration of I2.
The equilibrium constant (Keq) is defined as the ratio of the concentration of products to the concentration of reactants, each raised to their respective stoichiometric coefficients. For the given reaction:
I2(g) <-> 2I(g)
The equilibrium constant expression is:
Keq = [I]^2 / [I2]
Where [I] represents the concentration of I and [I2] represents the concentration of I2.
Given that Keq = 1.3 × 10^(-2) and [I2] = 0.0325, we can use this information to find the concentration of I.
Rearranging the equation, we get:
[I]^2 = Keq * [I2]
Substituting the values:
[I]^2 = (1.3 × 10^(-2)) * (0.0325)
Now, solving for [I]:
[I] = √[(1.3 × 10^(-2)) * (0.0325)]
[I] = √(4.225 × 10^(-4))
[I] ≈ 0.0206
Therefore, the concentration of I in the equilibrium mixture is approximately 0.0206.