Assume that in the analysis of another equilibrium mixture of the same reaction as above, at the same temperature of 448°C, the equilibrium concentrations of I2 and H2 are both 0.50 mol/L. What is the equilibrium concentrations of HI?
In order to determine the equilibrium concentration of HI, we need to use the balanced chemical equation and the equilibrium expression for the reaction:
2HI ⇌ H2 + I2
The equilibrium constant expression for this reaction is:
Kc = [H2][I2] / [HI]²
Since we are given the equilibrium concentrations of I2 and H2 as both 0.50 mol/L, we can substitute these values into the equilibrium constant expression:
Kc = (0.50)(0.50) / [HI]²
Since the equilibrium constant is a constant for a particular reaction at a given temperature, we can rearrange the equation to solve for [HI]:
[HI]² = (0.50)(0.50) / Kc
[HI]² = 0.25 / Kc
Taking the square root of both sides:
[HI] = √(0.25 / Kc)
Without knowing the specific value of the equilibrium constant Kc, we cannot determine the exact equilibrium concentration of HI.