Final answer:
The standard enthalpy of formation for nitromethane is 0 kJ/mol.
Step-by-step explanation:
To calculate the standard enthalpy of formation for nitromethane, we need to examine the balanced combustion equation given:
2CH₃NO₂(l) + 3/2 O₂(g) → ₂CO₂(g) + 3H₂O(l) + N₂(g).
The standard enthalpy of formation (ΔH°f) is the enthalpy change when one mole of a substance is formed from its elements in their standard states. By comparing the products and reactants in the equation, we can determine the change in enthalpy.
From the balanced equation, 2 moles of nitromethane (CH₃NO₂) are consumed to produce 2 moles of CO₂, which means the enthalpy change for this reaction is 0 kJ.
Therefore, the standard enthalpy of formation for nitromethane is 0 kJ/mol.