For the reaction: CH₃OH(g) + heat ↔ CO(g) + 2H₂(g) How will the equilibrium shift if the overall pressure is decreased?

-To the right
-To the left
- No effect

To the right

Explanation:

CH₃OH(g) + heat <=> CO(g) + 2H₂(g)

According to Le Chatelier's principle, a decrease in pressure will shift the equilibrium position to the side where there is a higher volume.

From the balanced equation above,

Volume of reactant = 1

Volume of product = 1 + 2 = 3

From the above, we can see that the volume of the gasous product is higher than the volume of the gasous reactant.

Therefore, a decrease in the pressure of the system will shift the equilibrium position to the right.

nacl is added to the aqueous of what? ? in order to get a proper answer you have to specify the exact composition of the aqueous solution.