Calculate the boiling point of a solution of 500.0 g of ethylene glycol (c2h6o2) dissolved in 500.0 g of water. kf = 1.86°c/m and kb = 0.512°c/m. use 100°c as the boiling point of water.

The boiling point of a solution of 500.0 g of ethylene glycol dissolved in 500.0 g of water is 108.258°C.

Explanation:

Elevation in boiling point :

= Boiling point of the solution

T = Boiling point of pure solvent

= Molal elevation constant of solvent

m = molality of the solution

Molality of the  ethylene glycol solution:

Moles of ethylene glycol =

Mass of solvent that uis water = 500.0 g = 0.5000 kg

Molal elevation constant of water =

Boiling point of the solution =

Boiling point of pure water = T = 100°C

The boiling point of a solution of 500.0 g of ethylene glycol dissolved in 500.0 g of water is 108.258°C.

idk i’m struggling too

m=9

step-by-step explanation: