How does the equilibrium between a solute and a solvent compare with the equilibrium between a liquid and its vapor?

Increase in pressure or concentration and decrease in temperature favors the formation of the liquid and the solute in the equilibrium between a liquid and its vapor and in the equilibrium between a solute and a solvent respectively.

Explanation:

In the equilibrium between a liquid and its vapor, as the pressure of the vapor increases it tends to favor the formation of the liquid, hence

Liquid ⇄ Vapor

By Raoult's law we have that the concentration of the components of an ideal mixture is proportional to the mole fraction and vapor pressure

That is

Also increase in temperature favors the formation of the vapor

Similarly the in the equilibrium between a solute and a solvent we have

While decrease in concentration results in an excess amount of solvent

So also, increase in the temperature of the solution results in the consumption of excess solute

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

the correct answer would be d. hope this !