Final answer:
The energy of 1 mol of gas at 100 degrees Celsius would depend on the heat capacity of the gas and cannot be exactly determined without additional information. For a monatomic ideal gas, using its molar heat capacity at constant volume, the estimated energy would be around 1247 J. For a phase change, such as vaporization of water, the energy is considerably higher, specifically 40.7 kJ.
Step-by-step explanation:
The energy content of 1 mol of gas at a certain temperature cannot be precisely determined without additional information, such as the type of gas and the process it is undergoing. However, if we are talking about ideal gases, we can use the heat capacity to estimate the energy. For example, the molar heat capacity at constant volume (CV) for a monatomic ideal gas is roughly 3/2 R, where R is the ideal gas constant (approximately 8.314 J/mol·K).
At 100 degrees Celsius (373 K), the energy for 1 mol of monatomic ideal gas would be Q = n·CV·ΔT = (1 mol)·(3/2)·(8.314 J/mol·K)·(373 K - 273 K) = 1·3/2·8.314·100 J ≈ 1247 J. For different types of gases or real gases, this calculation would require specific values of CV and could deviate from this estimate. Additionally, the energy required for phase changes, like vaporization of water, is specific heat and vastly different, being 40.7 kJ for 1 mol of water at 100°C.