DETERMINE THE NUMERICAL VALUE OF KEQ.
A) 2HI(g)--------H2(g) +I2(g)
Where [HI]=0.27m,[H2]=0.86M and [I2]=0.86M at 200c
Keq = (H2)(I2)/(HI)^2
Substitute and solve.
To determine the numerical value of Keq for the given reaction, you need to set up an expression for the equilibrium constant using the concentrations of the species at equilibrium. The general form of the equilibrium constant expression for a reaction is:
Keq = [products] / [reactants]
In this case, the reaction is:
2HI(g) ⇌ H2(g) + I2(g)
To calculate Keq, you need to determine the concentrations of each species at equilibrium. The given concentrations are:
[HI] = 0.27 M
[H2] = 0.86 M
[I2] = 0.86 M
Using the stoichiometry of the reaction, you can see that the concentration of H2 and I2 is the same. Therefore, you can assume that their concentrations are equal at equilibrium.
So, you can write:
[products] = [H2] * [I2] = (0.86 M) * (0.86 M) = 0.7396 M^2
[reactants] = [HI]^2 = (0.27 M)^2 = 0.0729 M^2
Now, you can substitute these values into the equilibrium constant expression:
Keq = [products] / [reactants] = 0.7396 M^2 / 0.0729 M^2
Calculating this mathematically, the numerical value of Keq for the given reaction is approximately 10.13.