The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g)...
The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium partial pressures of all species when H2 and I2, each at an intitial partial pressure of 1.65 atm, are introduced into an evacuated vessel at 698 K.
Homework Answers
H2(g) + I2(g) ---------------------- 2aT HI(g)
1.65 atm 1.65atm 0
-x -x +2x
1.65-x 1.65-x +2x
Kp = P^2HI/PH2xPI2
55.6 = (2x)^2/(1.65-x)x(1.65-x)
Square root of 55.6 = 2x/1.65-x
7.46 = 2x/1.65-x
12.309-7.46x = 2x
9.46x = 12.309
x= 12.309/9.46 = 1.30
x= 1.30 atm
At equilibrium
Partial pressure of H2= 1.65-x = 1.65-1.30= 0.35 atm
Partial pressureof I2 = 1.65-x = 1.65-1.30 = 0.35 atm
Partial pressure of HI = 2x = 2x1.30 = 2.60 atm.
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