Question

A 5 mole sample of liquid acetone is converted to a gas at 75.0°C. If 628 J are required to raise the temperature of the liquid to the boiling point, 15.600 kJ are required to evaporate the liquid, and 712 J are required to raise the final temperature to 75.0°C, what is the total energy required for the conversion?

Answer 1

The total energy required to convert a 5 mole sample of liquid acetone to gas at 75.0°C is 16,940 J or 16.940 kJ, which includes the energy to heat the liquid to the boiling point, vaporize it, and heat the vapor to the final temperature.

Step-by-step explanation:

The total energy required for the conversion of the liquid acetone to gas at 75.0°C can be calculated by summing up the individual amounts of energy needed for each step of the conversion process. The steps include raising the temperature of the liquid to its boiling point, vaporizing the liquid, and then raising the temperature of the vapor to the final temperature of 75.0°C.

Energy to raise the temperature to the boiling point: 628 J

Energy to vaporize the liquid (enthalpy of vaporization): 15.600 kJ or 15,600 J

Energy to raise the temperature of the vapor to 75.0°C: 712 J

To find the total energy, we simply add all these amounts together:

Total energy required = 628 J + 15,600 J + 712 J

Total energy required = 16,940 J or 16.940 kJ

Answer 2

The total energy required for this conversion is equivalent to the sum of the energies that are used. There are three steps:

1) Heating of liquid acetone
This used 628 J

2) Evaporation of acetone
This used 15.6 kJ or 15,600 J

3) Heating of acetone vapors
This used 712 J

Adding these quantities,

Total energy = 628 + 15,600 + 712

The total energy required was 16940 Joules of 16.94 kJ