Problem: 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.a. 0.327b. 0.701c. 2.03d. 1.42e. 1.88

FREE Expert Solution

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:

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Problem Details

The table below lists the equilibrium concentrations for H 2(g), I2(g), and HI(g) in the given reaction.

H(g) + I(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.

a. 0.327

b. 0.701

c. 2.03

d. 1.42

e. 1.88