Question

Calculate the equilibrium constant at 1000 K and 1 bar for the following gaseous phase reaction:

CO + H2O ↔ CO2 + H2

Data: K298 K = 1.1582×105

Answer 1

Answer:

Hey dear,

I assume you want to calculate partial pressure of CO or H2O

◆ Answer-

P(CO) = P(H2O) = 4.8 atm

◆ Explaination-

# Given-

Kp = 16

P(H2) = x = 1.2 atm

# Solution-

Let's arrange the reaction better -

Reaction CO2 + H2 ---> CO + H2O

Initially p p 0 0

Equilibrium p-x p-x x x

Equilibrium constant is given by-

Kp = [H2O][CO] / [CO2][H2]

Kp = (p-x)(p-x) / x.x

We have value of Kp and x,

16 = (p-1.2)(p-1.2) / (1.2)(1.2)

p-1.2 = 1.2 × 4

p = 6 atm

Therefore,

P(CO) = 6-1.2 = 4.8 atm

P(H2O) = 6-1.2 = 4.8 atm

Hope this helps...