2π»πΌ(π) β π»2
(π) + πΌ2(π)
πΎπΆ = 0.290 at 400 K. If the concentrations of HI, H2 and I2 are measured to be
1.50 Γ 10β3 M at 400 K, how will the system behave
To determine how the system will behave, we can compare the calculated reaction quotient (Qc) with the equilibrium constant (Kc).
The reaction quotient is calculated in the same way as the equilibrium constant, but using the initial concentrations of the reactants and products instead of the equilibrium concentrations.
The balanced equation for the reaction is:
2HI (g) β H2 (g) + I2 (g)
The initial concentration of HI is 1.50 Γ 10^β3 M, and the initial concentrations of H2 and I2 are both 0 M.
Therefore, the reaction quotient (Qc) is:
Qc = [H2][I2] / [HI]^2
= (0)(0) / (1.50 Γ 10^β3)^2
= 0 / 2.25 Γ 10^β6
= 0
Since Qc = 0 and Kc = 0.290, the system is not at equilibrium. This means that the reaction must proceed in the forward direction to reach equilibrium.
In other words, more HI will react to form H2 and I2 until the concentration of HI decreases and the concentrations of H2 and I2 increase.