As an AI language model, I cannot perform quantum chemistry calculations directly. However, I can provide you with the standard enthalpy of formation Hf of ethane C2H6 at room temperature 298K from literature values and guide you on how to perform quantum chemistry calculations.The standard enthalpy of formation Hf of ethane C2H6 at room temperature 298K is approximately -84.68 kJ/mol.To perform quantum chemistry calculations, you can use computational chemistry software packages like Gaussian, ORCA, or GAMESS. These programs use various quantum chemistry methods, such as Hartree-Fock HF , Density Functional Theory DFT , or post-Hartree-Fock methods like Mller-Plesset perturbation theory MP2 and Coupled Cluster CC theory.Here's a general outline of the process:1. Choose a suitable computational chemistry software package and install it on your computer or use an online platform that provides access to these tools.2. Create an input file for the software, specifying the molecular geometry of ethane C2H6 and the desired level of theory and basis set. For example, you might choose the B3LYP functional with a 6-31G d basis set.3. Run the calculation using the software. The program will perform a series of calculations to optimize the geometry and determine the electronic energy of the molecule.4. Calculate the enthalpy of formation Hf by subtracting the sum of the standard enthalpies of formation of the constituent elements 2C and 6H from the calculated electronic energy of ethane. You may need to convert the energy units to kJ/mol if they are not already in that format.5. Compare your calculated value to the literature value of -84.68 kJ/mol to see if your calculation agrees with the literature values.Keep in mind that the accuracy of your calculation will depend on the level of theory and basis set used. Higher levels of theory and larger basis sets generally provide more accurate results but require more computational resources.