Oxygen difluoride is a colorless, very poisonous gas that reacts rapidly and exothermically with water vapor to produce O2 and HF:
OF2 (g) +H20 (g) --> O2 (g) + 2HF (g) with delta H being -318 kJ.
What is the change in internal energy for the reaction of 1.00 mol OF2?
Do you assume that external pressure is constant unless it is explicitly stated that it changes? (because otherwise you can't use the ideal gas equation) And how are you supposed to use ideal gas equation to find change in internal energy?
I'm also confused as to why the question didn't mention the temperature of the reaction, since it's needed for the ideal gas equation.