May I get help on this?

Question

At a certain temperature, the equilibrium constant, 𝐾,K, for the given reaction is 53.3.

H2(g)+I2(g)↽−−⇀2HI(g)𝐾=53.3

At this temperature, the reactants were placed in a container to react. If the partial pressures of H2 and I2 were each 0.500 bar0.500 bar initially, what is the partial pressure of HI at equilibrium?

PHI= bar

Answer 1

Maybe best to use an ICE table to approach this problem

H₂(g) + I₂(g) ==> 2HI(g) ... K = 53.3

0.500....0.500..........0...........Initial

-x...........-x.............+2x.........Change

0.500-x...0.500-x....2x..........Equilibrium

K = (HI)² / (H₂)(I₂)

53.3 = (2x)2 / (0.5-x)(0.5-x)

53.3 = 4x² / x² -x +0.25

4x² = 53.3x² - 53.3x + 13.3

49.3x² - 53.3x + 13.3 = 0

x = 0.391 barr

Partial pressure of HI @ equilibrium = 2x = 2*0.391 barr = 0.782 barr