Final answer:
The energy released by condensing a given mass of water is indeed the same as that absorbed by evaporating the same mass of water. This is true because the processes of vaporization and condensation involve the same amount of energy transfer, but in opposite directions and is represented as Q = mLy, where Q is energy, m is mass, and Ly is the latent heat of vaporization/condensation.
Step-by-step explanation:
The statement that the energy released by condensing a given mass of water is the same as that absorbed by evaporating the same mass of water is True. When a substance changes from a liquid to a gas (vaporization), heat is absorbed from the surroundings, and energy is required to overcome the intermolecular forces within the liquid. Conversely, during condensation, the process is reversed and the gas turns back into a liquid, releasing the same amount of energy that was absorbed during vaporization. This energy exchange can be represented by the equation Q = mLy, where Q is the energy in joules, m is the mass in kilograms, and Ly is the latent heat of vaporization (or condensation).
The heat involved in the processes of vaporization and condensation is termed the latent heat of vaporization and condensation, respectively. As per the thermodynamic principle, the amount of energy change associated with the phase change is equal and opposite in sign for the two processes when the mass and the substance remain constant. Therefore, the molar heat of vaporization (AHvap) is numerically equal but opposite in sign to the molar heat of condensation (AHcond).