### Module: Equilibrium Part 3 Question 17

Posted:

**Mon Jan 06, 2020 9:41 pm**17. If the initial amounts of CO and H2O were both 0.100 M, what will be the amounts of each reactant and product at equilibrium for the following reaction? Keq = 23.2 at 600K

CO (g) + H2O (g) ⇌ CO2 (g) + H2 (g)

After using ICE, for my quadratic equation, I solved it from:

x^2 / (0.100 - x)^2 = 23.2

23x^2 - 4.64x + 0.232 = x^2

22x^2 - 4.64x + 0.232 = 0

However, using the quadratic formula, x turns out to be 0.126, which doesn't make sense because then the equilibrium concentration will be a negative number. Can someone tell me what I'm doing wrong?

CO (g) + H2O (g) ⇌ CO2 (g) + H2 (g)

After using ICE, for my quadratic equation, I solved it from:

x^2 / (0.100 - x)^2 = 23.2

23x^2 - 4.64x + 0.232 = x^2

22x^2 - 4.64x + 0.232 = 0

However, using the quadratic formula, x turns out to be 0.126, which doesn't make sense because then the equilibrium concentration will be a negative number. Can someone tell me what I'm doing wrong?