4D.7

[AlyssaYeh_1B]

"Oxygen difluoride is a colorless, very poisonous gas that reacts rapidly and exothermically with water vapor to produce O₂ and HF:

OF_{2 (g)} + H₂O_(g) ----> O_{2 (g)} + 2HF_(g) delta H = -318kJ

What is the change in internal energy for the reaction of 1.00 mol OF₂?"

I understand that we have to use the relationship between delta H and delta U, but the question doesn't provide a temperature. Are we supposed to assume that the reaction is taking place at room temp?

[Ronak Naik]

I think anytime there is no temperature we assume 25C (298K).

[Ronak Naik]

I think anytime there is no temperature we assume 25C (298K).

[Ritu Gaikwad 2E]

I would first look at pV=nRT for to solve for the temperature if all of that info is given but if not then I would just go with standard conditions at 298 K.

[005162520]

In what conditions is it not safe to assume that the temperature is not at room temperature besides when it is given?

[DHavo_1E]

Hi,

Could anyone explain how we know the net production of moles is 1.00 when it is stated as the reactant? Thank you!