Final answer:
The heat absorbed in the oxidation of 4.68L of nitrogen cannot be directly calculated without information on the enthalpy change of the reaction, as volume alone is insufficient for this determination in the context of a chemical reaction.
Step-by-step explanation:
The question "How much heat is absorbed in the oxidation of 4.68L of nitrogen gas measured at 1 atmosphere and 273 Kelvin?" cannot be answered directly with the information provided as there is no direct relation between the volume of gas used and the heat absorbed without knowing the apparent enthalpy change for the specific reaction involving nitrogen gas. This falls under a typical high school level chemistry problem where understanding of chemical reactions and thermodynamics is required.
To calculate heat absorbed using the ideal gas law, we need to know the specific heat of the substance and the change in temperature. This is not applicable in the case of a chemical reaction where the heat of reaction or enthalpy change is involved.
For calculation using enthalpy change, you would need to know the specific heat reaction for the oxidation of nitrogen. Without this, it's not possible to determine the heat absorbed. Typically, heat calculations involving chemical reactions make use of tabulated standard enthalpy changes or experimental data from calorimetry.