Calculate the freezing 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.

When a solute is added to a solvent, some properties are affected and these set of properties are called colligative properties. The properties depend on the amount of solute dissolved in a solvent. These properties include freezing point depression, boiling point elevation, osmotic pressure and vapor pressure lowering. For this case, we use freezing point depression:

 ΔT(freezing point)  = (Kf)m       where Kf is the freezing point depression constant and m is the molality

ΔT(freezing point)  = 1.86 °C kg / mol (500 g c2h6o2 ) ( 1 mol / 62.08 g ) / 0.500 kg water 

ΔT(freezing point)  = 29.96 °C
Tf - T = 29.96 °C
T = -29.96 °C

Therefore, the freezing point of the solution of ethylene glycol is -29.96 °C

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8