An ethylene glycol solution contains 25.2 g of ethylene glycol (C₂H₆O₂) in 99.5 mL of water. Determine the change in boiling point. Assume a density of 1.00 g/mL for water.

• A. 18.4°C
• B. 9.22°C
• C. 2.08°C
• D. 0.572°C

Answer: (C)

Verified step by step guidance

1. Calculate the molar mass of ethylene glycol (C2H6O2) by adding the atomic masses of its constituent elements: carbon (C), hydrogen (H), and oxygen (O).
2. Determine the number of moles of ethylene glycol by dividing the mass of ethylene glycol (25.2 g) by its molar mass.
3. Calculate the mass of water in grams using the given volume (99.5 mL) and the density of water (1.00 g/mL).
4. Find the molality of the solution by dividing the moles of ethylene glycol by the mass of water in kilograms.
5. Use the boiling point elevation formula, ΔT_b = i * K_b * m, where i is the van't Hoff factor (1 for ethylene glycol), K_b is the ebullioscopic constant for water, and m is the molality, to calculate the change in boiling point.