Relationship in equilibrium constants $\ce{2CH4(g) + O2(g) \rightleftharpoons 2CO(g) + 4H2(g)}$


  Equal numbers of moles of $\ce{CH4}$ and $\ce{O2}$ are drawn into a
  sealed container and the system is left until it reaches equilibrium.
  Which of the following relationships pertaining to this particular
  system are true at equilibrium?
  
  
  $\ce{[CH4]&lt;[H2]}$
  $\ce{[CH4]&gt;[O2]}$
  $\ce{[H2]&gt;[CO]}$
  


I know that the equation for $\ce{K_{eq}}$ is

$$\ce{\dfrac{[H2]^4[CO]^2}{[CH4]^2[O2]}}$$

I think that 3. is wrong because if $\ce{CH4}$ and $\ce{O2}$ are equal, then $\ce{H2}$ and $\ce{CO}$ have to be the same. Now I'm confused about 1 and 2. I'm not sure how to distinguish between the two.
Let's say that the amount of $\ce{CH4}$ and $\ce{O2}$ at the start is $x$.

After the reaction is complete, let's say that $y$ moles of $\ce{O2}$ reacted.

The amount of moles of $\ce{CH4}$ left is $x-2y$;

The amount of moles of $\ce{O2}$ left is $x-y$;

The amount of moles of $\ce{CO}$ formed is $2y$;

The amount of moles of $\ce{H2}$ formed is $4y$;

That should make one of the choices clearly false, one clearly true and one might not be so obvious, unless you assume that the forward reaction path is less favourable ($\ce{CO}$ is not very stable)