We’re being asked to calculate the equilibrium concentration of I_{2}, given the following reaction:

H_{2}(g) + I_{2}(g) ⇌ 2 HI(g).; **K _{p} = 54**

We're given the equilibrium pressures:

P_{H2} = 0.712 atm

P_{I2} = ?

P_{HI} = 2.77 atm

The **K _{p} expression** for the reaction is:

At 700 K, the reaction below has an K_{p} value of 54. An equilibrium mixture at this temperature was found to contain 0.712 atm of H_{2} and 2.77 atm of HI. Calculate the equilibrium pressure of I_{2}.

H_{2}(g) + I_{2}(g) <=> 2 HI(g). Enter to 2 decimal place.

a. 0.07 atm

b. 0.20 atm

c. 581.93 atm

d. 19.95 atm

e. 210.08 atm

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