5 votes
Accepted

Total entropy change for reversible reactions and its relationship to equilibrium constant

For points 1 and 3, if they're both agreed to be true then $\Delta S_{\text{total}} = 0=R\ln K \implies K = 1$, no matter the reaction. The entropy change of a reaction is concentration-dependent: $$\...
  • 32.7k
3 votes

Le Chatelier's Principle - Increasing concentration of coloured ion

If $\ce{CoCl2·6H2O}$ is dissolved in water, the solution is pink, because of the pink ion $\ce{[Co(H2O)6]^2+}$. Matter of fact, the amount of blue $\ce{CoCl4^2-}$ ion produced by the following ...
  • 22.5k
3 votes

Why does CaSO4 break up when adding HCl but not BaSO4?

Sulphates of alkali earth metals dissolve like this: $$\ce{MSO4(s) <=>[H2O] M^2+(aq) + SO4^2-(aq)}\tag{1}$$ with the solubility product constant (kept original eq. numbering): $$K_\mathrm{sp} = ...
  • 29.7k
3 votes

Total entropy change for reversible reactions and its relationship to equilibrium constant

(1) The entropy reaches a maximum at equilibrium, thus any change will depart from equilibrium, but this cannot happen if we are at equilibrium unless some other parameter changes such a temperature ...
  • 27.6k
2 votes

Schlögl model - Stationary States far from Equilibrium

[my comment] There are two stable equilibria. There are details and a clear discussion in MIra et al. J. Chem. Educ. 2003, v80, p1488, also a v. thorough explanation in D. Gillespie, 'Markov Processes'...
  • 27.6k
1 vote

Can a weak acid ever fully dissociate?

Strictly speaking, no acid is fully ionized in water solutions. Even strong acid solution has traces of a not dissociated forms, as their acidity constants are very high, but not infinite. For all ...
  • 29.7k
1 vote

chemical equilibrium and activity

The $\ce{Ba^{2+}}$ ions will surround by anions The $\ce{SO_4^{2-}}$ will be surrounded by cations So they stabilize a lot more actually. Remember that this may take long, but thermodynamically that ...
  • 19

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