Chapter 9 Problem 43

Volume:
Temperature:

Moderators: Chem_Mod, Chem_Admin

E_Villavicencio 2N
Posts: 26
Joined: Wed Sep 21, 2016 2:59 pm

Chapter 9 Problem 43

Postby E_Villavicencio 2N » Tue Jan 31, 2017 4:40 pm

In the solution of this problem, we have to consider two samples of water that were mixed and obtain the change in entropy. However, when we have to use the formula delta S=nCln(T2/T1) the solution manual uses 75.3 J/K as the heat capacity of water. Can someone explain to me where that value came from? Why don't we use 4.184J/K?

Chem_Mod
Posts: 18400
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 435 times

Re: Chapter 9 Problem 43

Postby Chem_Mod » Tue Jan 31, 2017 8:36 pm

So the simplest solution to your question is that this is the exact same value.

If you take and multiply it by water's molar mass of 18.02 g/mole, you get

In addition, it is found in Table 9.2 of the book on pg334


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

Who is online

Users browsing this forum: No registered users and 1 guest