November 27, 2024, 05:41:45 PM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Calcium acetate + heat?  (Read 2966 times)

0 Members and 1 Guest are viewing this topic.

Offline xXCuteGoatXx

  • New Member
  • **
  • Posts: 8
  • Mole Snacks: +0/-0
Calcium acetate + heat?
« on: January 08, 2018, 04:33:10 PM »
Hi!

Plain and simple; I'm wondering why calcium acetate breaks down to calcium carbonate and acetone when heated.

Thank you.
Logged

Offline wildfyr

  • Global Moderator
  • Sr. Member
  • ***
  • Posts: 1776
  • Mole Snacks: +203/-10
Re: Calcium acetate + heat?
« Reply #1 on: January 08, 2018, 07:05:56 PM »
Plain and simple? Entropy.

Two gas molecules are better than 1 salt molecule.
Logged

Offline xXCuteGoatXx

  • New Member
  • **
  • Posts: 8
  • Mole Snacks: +0/-0
Re: Calcium acetate + heat?
« Reply #2 on: January 08, 2018, 07:11:57 PM »
Quote from: wildfyr on January 08, 2018, 07:05:56 PM
Plain and simple? Entropy.

Two gas molecules are better than 1 salt molecule.

No, I meant that my question was plain and simple. Please exuse my English..

I'd love a more detailed explaination.

Thank you.
Logged

Offline MangoPaws

  • New Member
  • **
  • Posts: 6
  • Mole Snacks: +1/-0
Re: Calcium acetate + heat?
« Reply #3 on: January 09, 2018, 09:21:21 AM »
The acetate ions are oxidisable and reducible. Here the two in the salt disproportionate, one is oxidised to carbonate, one reduced to acetone. The acetone is released increasing entropy of the process and the potentially the carbonate salt has an increased lattice enthalpy so the process is spontaneous when head is applied.
Logged
Pages: [1]   Go Up
« previous next »
Sponsored Links