## 4D.7

AlyssaYeh_1B
Posts: 100
Joined: Sat Aug 17, 2019 12:16 am

### 4D.7

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

OF2 (g) + H2O(g) ----> O2 (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
Posts: 103
Joined: Sat Jul 20, 2019 12:15 am

### Re: 4D.7

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

Ronak Naik
Posts: 103
Joined: Sat Jul 20, 2019 12:15 am

### Re: 4D.7

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

Posts: 52
Joined: Thu Jul 11, 2019 12:16 am

### Re: 4D.7

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
Posts: 101
Joined: Tue Sep 24, 2019 12:17 am

### Re: 4D.7

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

DHavo_1E
Posts: 118
Joined: Sat Aug 17, 2019 12:17 am

### Re: 4D.7

Hi,

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

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