When one mole of ch3oh (l) forms from its elements at 1 atm and 25 degrees c, 238.6 kj of heat are released, and 35.2 kj are released when one mole of the gas condenses. how much heat is released when one mole of ch3oh (g) forms from its elements at these conditions?

So, the first thing I would do is underline the important parts of the question. 
(I'm going to capitalize what I think is important just so I can understand fully too hahaha)

It's asking you for ONE MOLE of CH3OH (l) and that 238.6 KJ are RELEASED. Making this equation an exothermic reaction. 
It also says that 35.2 KJ are released when ONE MOLE of GAS condenses, another exothermic reaction.
Then, they want you to find out how much heat is released the ONE MOLE of CH3OH (g) forms from the elements

You then need to figure out what equation to use, how I see it, the best equation to use for one mole of CH3OH would be

CO+ 2H2> CH3OH (l) H= -238.6 (since its releasing energy)

The second equation would be 
CH3OH (g)> CH3OH (l) H= -35.2 (also releasing energy) 

The final equation it wants is one mole of CH3OH (g)
CO + 2H2> CH3OH (g) H= ?

The first main step is to look at all of your equations and see what needs to be changed. From what I can see, the CH3OH (g) would need to be flipped to the other side because it's on the same side as your CO + 2H2> CH3OH (l) equation at the top. 

You do this by multiplying by a -1, so the equation would look like this
-1 (CH3OH (g)> CH3OH (l) H= -35.2 KJ)
CH3OH (l)>CH3OH (g) H= 35.2 KJ

You can then cross cancel out the CH3OH (l) since they are on opposite sides and are not part of the end equation. You can then combine the remaining elements

You are then left with CO + 2H2> CH3OH (g)

You can then solve for the heat of CH3OH by adding your new H numbers, so simply add (-238.6) + (35.2) = -203.4

And that should be your answer!
Hope this helped, if not I am so sorry!