How many grams of ethylene glycol (c2h6o2) must be dissolved in 200 grams of water to lower the freezing point to -29.75 Celsius? if the density of ethylene glycol is 1.12g/m1, how many milliliters of ethylene glycol are required?

mass of ethylene glycol = 198. 562 g

Volume of ethylene glycol = 177.2875 ml

Explanation:

The freezing point depression of the solvent can be expressed by the formula:

where

= molar freezing point depression constant of water = 1.86 °C/m

= freezing point depression = 0°C -(-29.75°C)

    = 29.75°C

m = molarity of ethylene glycol

i = the value of Van't Hoff Factor = 1

replacing our value into above expression; we have:

m = 15.995 M

Also. Molarity =

mass of ethylene glycol = 198. 562 g

Density =

Given that;

the density of ethylene glycol is 1.12g/ml

and our derived mass of ethylene glycol = 198. 562 g; we can determine how many milliliters of ethylene glycol  are required by calculating the volume

Volume of ethylene glycol =

Volume of ethylene glycol =

Volume of ethylene glycol = 177.2875 ml

it means there are 3 atoms of oxygen