How many grams of ethylene glycol (c2h6o2) must be added to 1.05 kg of water to produce a solution that freezes at -4.66 ∘c?

163g of ethylene glycol

Explanation:

The addition of a non-volatile solute to a solvent as water produce the decreasing of freezing point following the formula:

ΔT = Kf×m×i

Where ΔT is change in freezing point (0°C- (-4.66°C) = 4.66°C); Kf is freezing point depression constant (1.86°C/m); m is molality (moles of solute / kg solvent); i is Van't Hoff factor (1 for ethylene glycol in water)

Replacing:

4.66°C = 1.86°C/m × moles solute / 1.05kg

2.63 = moles solute.

Molar mass of ethylene glycol is:

C: 12.01×2 = 24.02g/mol

H: 6×1.01 = 6.06g/mol

O: 2×16 = 32g/mol

24.02g/mol + 6.06g/mol + 32g/mol = 62.08g/mol

Thus, mass of ethylene glycol must be added is:

2.63mol × (62.08g/mol) = 163g of ethylene glycol

specific gravity is the density of a substance divided by the density of water. since (at standard temperature and pressure) water has a density of 1 gram/cm3, and since all of the units cancel, specific gravity is usually very close to the same value as density

so "c" is the answer

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the volume increases