Question #02a40

Oct 28, 2017

Dynamic equilibrium is the idea that while the concentrations of product and reactant do not change, the reaction is still happening.

Explanation:

Dynamic equilibrium is essentially this idea that while the concentrations of product and reactant do not change, the reaction is still happening. In other words, the reaction does not just "stop" once you reach equilibrium.

For example, consider the acid-dissociation reaction for acetic acid $\left(C {H}_{3} C O O H\right)$:

$C {H}_{3} C O O {H}_{\left(a q\right)} + {H}_{2} {O}_{\left(l\right)} r i g h t \le f t h a r p \infty n s C {H}_{3} C O {O}_{\left(a q\right)}^{-} + {H}_{3} {O}_{\left(a q\right)}^{+}$

When this reaction reaches a certain point, the concentrations of product and reactant will cease to change. However, the reaction will continue to keep going on.

Make sure you understand this idea well; it is a favorite test question for many teachers.

If you still don't get the concept, here's some great videos you could check out:
Bozeman Science - "Equilibrium"
Michael Evans - "The Equilibrium State"

Hope that helped :)