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

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explanation:

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rvmoo+478)9.68

answer is: c. the experiment shows that the red substance experienced a chemical change.

this is chemical change (chemical reaction), because two new substances are formed (metalig liquid and gas), the atoms are rearranged and the reaction is followed by an energy change.

this is example of chemical decomposition.

chemical decomposition (analysis) is the separation of a single chemical compound into its two or more elemental parts or to simpler compounds.  

chemical decomposition is opposite of chemical synthesis.