Oxygen difluoride is a colorless, very poisonous gas that reacts rapidly with wa

Question

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

OF2 (g) + H2O (g) -> O2 (g) + 2HF (g)

delta H = -318 KJ

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

Here is the work I got done so far:

delta n = +1 mol

PV=nRT

PdeltaV=deltanRT

-PdeltaV=-deltanRT= -(1mol)(8.314 J/kmol)*T

according to my textbook, T=298K. How do I figure out that T=298K on my own and why is T=298K. I want to learn the process by which T is determined.

Explanation / Answer

T is taken to be normal room temperature i.e. 25 C which is 298K. We dont have to calculate it

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