[digisol]

Is this textbook answer wrong? Here is the problem:

The equilibrium constant at 25 C for the reaction CO2(g) + H2(g) -> H2O(l) + CO(g) is 3.22 x 10^-4. What pressures of CO2 and H2 are needed to produce CO at a pressure of 0.100 atm? Take the pressures of CO2 and H2 to be equal, and assume that all the gases obey the ideal gas law.

My attempt:
K = P(CO) / (P(H2) * P(CO2))
Since P(H2) = P(CO2):
K = P(CO) / P(H2)^2
Rearranging:
P(H2)^2 = P(CO) / K
P(H2) = sqrt(P(CO) / K) = sqrt(0.1 atm / 3.22 x 10^-4) = 17.6 atm

The book gives the answer as 55.7 atm. Which is correct?

[Borek]

Must be a typo, 55.7 is a correct answer for CO pressure of 1 atm.

[digisol]

Thank you!