Final answer:
The difference between the calculated and measured molar heat capacities of gases at 298K can be attributed to changes in internal energy. Calculations are based on theoretical assumptions, while measurements are obtained through experiments.
Step-by-step explanation:
The difference between the calculated and measured molar heat capacities of gases at 298K can be attributed to changes in internal energy. Calorimetry is a technique used to measure heat changes during chemical processes. The molar heat capacity (c) represents the amount of energy needed to raise the temperature of 1 mole of a substance by 1°C.
When calculating the molar heat capacity, it is important to consider enthalpy, entropy, and internal energy. Enthalpy (ΔH) represents the amount of heat released or absorbed during a reaction at constant pressure. Entropy (ΔS) measures the amount of disorder or randomness in a system. Internal energy (ΔU) reflects changes in both enthalpy and entropy.
In relation to the measured and calculated molar heat capacities, the difference can be attributed to experimental errors or variations in the system. Calculated values are based on theoretical calculations and assumptions, while measured values are obtained through experimental observations. These differences can arise due to limitations in measurement techniques, instrumentation, or the inherent complexity of the system being studied.