Consider the following reversible reaction:
$CO(g)+2 H_2(g) \longleftrightarrow CH_3 OH(g)$
What is the equilibrium constant expression for the given system?
A$K_{e q}=\frac{\left[CH_3 OH\right]}{[CO]\left[H_2\right]}$
B$K_{eq}=\frac{[CO]\left[H_2\right]}{\left[CH_3 OH\right]}$
C$K_{e q}=\frac{\left[CH_3 OH\right]}{[CO]\left[H_2\right]^2}$
D$K_{e q}=\frac{CO\left[H_2\right]^2}{\left[CH_3 OH\right]}$
$CO(g)+2 H_2(g) \longleftrightarrow CH_3 OH(g)$
What is the equilibrium constant expression for the given system?
A$K_{e q}=\frac{\left[CH_3 OH\right]}{[CO]\left[H_2\right]}$
B$K_{eq}=\frac{[CO]\left[H_2\right]}{\left[CH_3 OH\right]}$
C$K_{e q}=\frac{\left[CH_3 OH\right]}{[CO]\left[H_2\right]^2}$
D$K_{e q}=\frac{CO\left[H_2\right]^2}{\left[CH_3 OH\right]}$