Final answer:
The boiling point of a 16% aqueous solution of ethylene glycol will be higher than 100°C, the boiling point of pure water, due to boiling point elevation. The precise boiling point cannot be calculated without additional information.
Step-by-step explanation:
The subject of this question relates to the boiling point elevation of an aqueous solution due to the presence of a solute, specifically ethylene glycol (C2H6O2) in water. The boiling point elevation can be calculated using the formula ΔTb = i * Kb * m, where ΔTb is the change in boiling point, i is the van't Hoff factor (which is 1 for ethylene glycol as it does not ionize in solution), Kb is the ebullioscopic constant for water (0.51 C m-1), and m is the molality of the ethylene glycol solution. To find the molality, we need to know the number of moles of ethylene glycol and the mass of the solvent (water) in kilograms.
However, since the student question does not provide enough information to calculate the precise boiling point elevation (such as the total mass of the solution or the mass of water), a general statement can be made that the boiling point of the 16% ethylene glycol solution will be higher than the boiling point of pure water, which is 100°C at standard atmospheric pressure.