Chapter 13, Problem 100CP

A 4.72-g sample of methanol (CH₃OH) was placed in an otherwise empty 1.00-L flask and heated to 250.°C to vaporize the methanol. Over time, the methanol vapor decomposed by the following reaction:

${\text{CH}}_3\text{OH}\left(g\right)\rightleftharpoons \text{CO}\left(g\right)+2{\text{H}}_2\left(g\right)$

After the system has reached equilibrium, a tiny hole is drilled in the side of the flask allowing gaseous compounds to effuse out of the flask. Measurements of the effusing gas show that it contains 33.0 times as much H₂(g) as CH₃OH(g). Calculate K for this reaction at 250.°C.