9.45 Help.


Moderators: Chem_Mod, Chem_Admin

Andrew Uesugi 3I
Posts: 38
Joined: Wed Sep 21, 2016 2:56 pm

9.45 Help.

Postby Andrew Uesugi 3I » Sun Jan 29, 2017 3:58 pm

So the question is asking me this:

Calculate the changes in entropy of the surroundings and of the system for (a) the vaporization of 1.00 mol CH4 at is normal boiling point.

So I know the formula is Delta S = - Delta H / T. Why is T = 111.7 K?

Hao 1I
Posts: 26
Joined: Wed Sep 21, 2016 3:00 pm
Been upvoted: 1 time

Re: 9.45 Help.

Postby Hao 1I » Sun Jan 29, 2017 8:18 pm

The temperature is 111K because that is the boiling point for CH4. The equation for change in entropy for vaporization is equal to the enthalpy of vaporization divided by the boiling point temperature ( delta S = delta H of vaporization / Temp. at boiling point ).

Return to “Entropy Changes Due to Changes in Volume and Temperature”

Who is online

Users browsing this forum: No registered users and 2 guests