Increasing the molality of a solution the boiling point of a solution. Changing the solute to one that creates fewer dissolved species the boiling point of the solution compared to the original solution. Starting a solution at a warmer temperature the boiling point of a solution.

-Increase the boiling point

-Decrease the boiling point

- Will not change

Explanation:

The boiling point of a solution is the temperature at which its vapor pressure equals the external atmospheric pressure.

Because the presence of a nonvolatile solute lowers the vapor pressure of a solution, it also affects the boiling point of the solution. Remember that molality is a concentration unit that is obtained by dividing the moles of solute in one kilogram of solvent. Increasing the molality, that is, increasing the amount of solute in a solution, will increase the boiling point of a solution. This is an example of a colligative property, a property that depends only on the number of solute particles in solution and not on the nature of the solute particles. Because of this same reason, changing the solute to one that creates fewer dissolved species, which are the ones that will exert their effects in the solution, will decrease the boiling point compared to the original solution, since here there are fewer particles in solution.

Since the definition of boiling point states that it is a temperature at which vapor pressures are equal, starting a solution at a warmer temperature will not change the boiling point, it will just take less time to reach that same boiling point.

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"