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Is there any specific definition of position of equilibrium? … Note that K is the equilibrium constant, not "the equilibrium". A condition of chemical reaction equilibrium is that Q=K. …

On nomenclature: thermodynamic changes ($\Delta G^\circ$, $\Delta H^\circ$ etc) refer to processes between equilibrium states, an initial equilibrium state and a final equilibrium state. … This is why the field is called equilibrium thermodynamics. …

The equilibrium constant is a concentration equilibrium constant. … As this final concentration of C is inconsistent with an equilibrium point, we can logically conclude that $\pu{[B]= 3 M}$ cannot be achieved. …

A cursory search suggests the solubilities in g/100 mL on the wikipedia are closer to a consensus, for what it's worth: solubility 0.2% ($0^oC$): https://www.cdc.gov/niosh/npg/npgd0092.html solubi …

This problem is relatively easy to solve if you remember that the vapor pressure of the products is independent of the amount of solid, provided there is enough solid for it to be in equilibrium with the …

The following shows more formally how to derive the connection between Henry's law, an equilibrium constant and the standard Gibbs free energy for evaporation of the solute. … constant for the equilibrium $\ce{solute <=> gas}$ provided we define the equilibrium constant as $$K_{eq} = \frac{K}{p^\circ } = \frac{p_i/p^\circ}{m_i/m^\circ }$$ …

{n_A n_B}\right) \\&= \Delta \mu^* + RT \ln \left(\frac{\chi_C}{\chi_A \chi_B}\right) \end{align} $$ ($^\dagger$) Note that here the standard state for each substance refers to the pure liquid in equilibrium … To obtain an expression relating a change in standard free energy to the concentration equilibrium constant requires expressing mole fractions in terms of concentrations. …

It's sometimes not obvious because of the way the subject may be taught, but $\Delta_rG$ is what's called a differential form, so it actually describes how the free energy changes as the reaction prog …

There are a few different ways to derive the van't Hoff equation. The question here however is to justify the mathematical form of the equation. A good (if not entirely satisfying) way to do so is to …

If a reagent with constant activity is exhausted before equilibrium is reached the reaction stops - it is then a limiting reagent. … If a reaction is already at equilibrium, adding more of a solid won't make a difference (provided there are no surface effects). …

The autoionization equilibrium of water is satisfied irrespectively of $\mathrm p\ce{H}$. … mathrm p\ce{H} + \mathrm p\ce{OH}$$ This is a bit different from the typical scenario in which Le Chaterlier's principle is invoked because $\ce{H3O+}$ and $\ce{OH-}$ are on the same side in the reaction equilibrium …

Its value depends on the specified reference standard states and $T$ (and obviously on the equilibrium activities of reactants and products). … You can also compute an equilibrium constant from a value of $\Delta G^\circ$. …

We often need to distinguish between "real equilibrium states" and "kinetically trapped or metastable states". … Again, the definition of equilibrium is not as strict as we'd like to think. …

A variety of models have been concocted to describe the dependence of gas-phase reaction rates on the energy of collisions between two molecules. At its simplest you have the empirical Arrhenius equat …

You can relate an equilibrium constant $K_p$ written in terms of partial pressures to one written in terms of mole fractions $K_\chi$, as follows: $$K_\chi=K_p (p/p_0)^{-\Delta \nu}\tag{1}$$ where $\ …