Simultaneous Equilibrium Reactions, One Goes to Completion
Initially

Suppose that initially, before any reaction, these are the species and amounts present:

$$\ce{CH4}: m \textrm{ moles} $$
$$\ce{H2O}: w \textrm{ moles} $$
$$\ce{C2H6}: e \textrm{ moles} $$
$$\ce{H2}: h \textrm{ moles} $$
$$\ce{CO}: c \textrm{ moles} $$

After the second reaction completes

Let's assume that the second reaction is limited by the amount of ethane present, not the amount of water.  (This must be true, otherwise the first reaction could not be at "equilibrium" because one of the equilibrating species would  head to a concentration of zero.)  If the reaction is limited by ethane, then when it completes, $2e$ moles of carbon monoxide and $5e$ moles of hydrogen are formed.

$$\ce{CH4}: m \textrm{ moles} $$
$$\ce{H2O}: w - 2 e \textrm{ moles} $$
$$\ce{C2H6}: 0 \textrm{ moles} $$
$$\ce{H2}: h + 5e\textrm{ moles} $$
$$\ce{CO}: c + 2e\textrm{ moles} $$

After the first reaction equilibrates

The first reaction doesn't go to completion.  Instead, let's assume the extent of the reaction from our current state to the equilibrated state is $\xi$ moles.  That means that the species inventory becomes:

$$\ce{CH4}: m - \xi \textrm{ moles} $$
$$\ce{H2O}: w - 2 e - \xi \textrm{ moles} $$
$$\ce{C2H6}: 0 \textrm{ moles} $$
$$\ce{H2}: h + 5e + 3 \xi \textrm{ moles} $$
$$\ce{CO}: c + 2e + \xi \textrm{ moles} $$

These values can now be plugged into an equilibrium equation:

$$ K = \frac{[\ce{H2}]^3 [\ce{CO}]}{[\ce{CH4}][\ce{H2O}]}$$

$$ K = \frac{(h + 5e + 3 \xi)^3(c + 2e + \xi)}{(m-\xi)(w - 2 e - \xi)} $$

Now "all" you have to do is solve that equation for $\xi$.