Calculating an equilibrium constant from a partial equilibrium composition

$\frac{0}{5}$

Steam reforming of methane $(C{H}_4)$ produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a $50\mathrm{.}0L$ tank with $23.$ mol of methane gas and $8\mathrm{.}0$ mol of water vapor, and when the mixture has come to equilibrium measures the amount of carbon monoxide gas to be $1\mathrm{.}6$mol.

Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to $2$ significant digits.