A mixture of H2 and I2 is allowed to react at 448°C. When equilibrium is established, the concentrations of the participants are found to be [H2] = 0.46 mol/L, [12]=0.39 mol/L, and [HI] = 3.0 mol/L. Calculate the value of the Keq at 448°C.
H2(g) + 2(g)<=====> 2 HI(g)
For the given reaction:
H2(g) + I2(g) <=> 2 HI(g)
The equilibrium constant (Keq) can be calculated using the concentrations of the participants at equilibrium. The formula for Keq is:
Keq = ([HI]^2) / ([H2] * [I2])
Given the concentrations at equilibrium:
[H2] = 0.46 mol/L
[I2] = 0.39 mol/L
[HI] = 3.0 mol/L
Plugging these values into the equation for Keq:
Keq = (3.0^2) / (0.46 * 0.39)
Keq = 9.0 / 0.1794
Keq ≈ 50.14
Therefore, the value of Keq at 448°C is approximately 50.14.