H2 + I2 <====> 2 HI.
Looking for Keq:
Complete the equation. Assume all concentrations are equilibrium constants in mol/L , M
Temp in Celcius = 25
[H2] = .355
[I] = .388
[HI] = .0922
K eq = ??
Note the correct spelling of celsius.
Keq = (HI)^2/(H2)(I2)
Substitute and calculate.
6.17
To find the equilibrium constant Keq for the given reaction, we need to use the concentrations of the reactants and products. The equilibrium constant expression for the reaction is:
Keq = [HI]² / ([H2] * [I2])
We are given the following concentrations:
[H2] = 0.355 M
[I2] = unknown (to be determined)
[HI] = 0.0922 M
We need to find the concentration of I2 to calculate Keq.
Since the reaction stoichiometry is 1:1:2 (H2:I2:HI), we can determine the concentration of I2 using the concentration of HI.
From the given reaction equation, we can see that the number of moles of HI formed is twice the number of moles of I2 consumed. Therefore, the equilibrium concentration of I2 is half of the equilibrium concentration of HI:
[HI] = 0.0922 M
[I2] = [HI] / 2
= 0.0922 M / 2
≈ 0.0461 M
Substituting the values of [HI] and [I2] into the Keq expression, we have:
Keq = (0.0922 M)² / (0.355 M * 0.0461 M)
= 0.00848 / 0.01636
≈ 0.517
So, the equilibrium constant Keq for the given reaction is approximately 0.517.