Final answer:
The calculation requires the molar heat of combustion for ethylene glycol which is not provided in the question or reference information. Once obtained, the heat required can be calculated, and then the moles and mass of ethylene glycol required to produce this heat can be determined.
Step-by-step explanation:
To determine the mass of ethanediol (ethylene glycol) that must be burned to raise the temperature of 250 g of water from 20°C to 35°C, the specific heat of water and the total heat needed for the temperature change must be considered. First, let's calculate the heat required using the formula:
q = m × c × ΔT
where q is the heat in joules, m is the mass of water in grams (250 g), c is the specific heat capacity of water (4.18 J/g°C), and ΔT is the change in temperature in degrees Celsius (35°C - 20°C = 15°C).
Using these values:
q = 250 g × 4.18 J/g°C × 15°C
q = 15,675 J
The molar heat of combustion of ethylene glycol can be obtained from a reference or previous experiment. We do not have this value given, but as an example, let's assume it is X kJ/mol. We can then calculate the moles of ethylene glycol required to produce 15,675 J and then convert this to mass using the molar mass of ethylene glycol (62.07 g/mol).
Since the specific molar heat of combustion of ethylene glycol is not provided in the question, nor in the reference information given, and is needed to answer this question accurately, we cannot proceed with the calculation. The student might need to refer to experimental data or a credible data source to find the molar heat of combustion for ethylene glycol to complete the calculation.