Question

chem

Answer 1

i don't know how to start

Answer 2

Do you know how colligative properties work? Do you know the formula you are to use?

Answer 3

@aaronq no my book is pretty bad at e xplaining.

Answer 4

Colligative properties arise from the use of a non-volatile solute in a solvent - in your example ethylene glycol is the solute and water is the solvent.

By adding solute, you can raise the BP of a solution. This happens because particles of solute at the solvent-air interface physically block solvent molecules from entering the gas phase - this lowers the vapour pressure of the solution. The more solute you add the higher the BP will be.

The formula you are to use is \(\Delta T =i*m*K_b\)

where \(\Delta T\) is the change in temperature (from the pure solvent)
\(i\) is the van't hoff constant
\(m\) is the molality
\(K_b\) is the boiling point elevation constant specific to a solvent

Answer 5

yeah first calculate molality of the solution like
molality=weight of solute/molar mass of solute

Answer 6

that's not the molality equation

\(\sf molality=\dfrac{moles_{solute}}{kg_{solvent}}=\dfrac{\dfrac{mass~of~solute}{Molar~mass~of~solute}}{kg_{solvent}}\)

Answer 7

After that find the change in freezing point

\[\Delta Tf = i(Kfm) \]

Answer 8

ok calculate first what's formula wt for ethylene glycol....

Answer 9

thats not right. Break it up into steps if it's easier.


First find the moles of solute; \(\sf moles=\dfrac{mass}{molar~mass}\)