We’re being asked to calculate the equilibrium constant for the reaction:
H2(g) + I2(g) ⇌ 2 HI(g);
We're given the equilibrium pressures:
PH2 = 0.467 atm
PI2 = 0.467 atm
PHI = 0.666 atm
The Kp expression for the reaction is:
The table below lists the equilibrium concentrations for H 2(g), I2(g), and HI(g) in the given reaction.
H2 (g) + I2 (g) ⇌ 2HI (g)
The equilibrium partial pressures observed when the reaction comes to equilibrium at 720 K are PI2 = 0.467, PH2 = 0.467, and PHI = 0.666. What is the equilibrium constant for the reaction at this temperature? Please circle your answer.