Hello, just want to share a helpful "push and pull" analogy that the TA gave during an earlier discussion sections.
When something is added to one side of the equation (ex: increase concentration of reactant), it will "push" the equation to the other side (shift right, product increase).
When something is taken away from one side of the equation (ex: decrease concentration of reactant), it will "pull" the equation to its side (shift left, reactant increase.
This was super helpful for me to visualize Le Chatelier's principle :D
helpful "Push and Pull" Analogy
Moderators: Chem_Mod, Chem_Admin
Re: helpful "Push and Pull" Analogy
This was a great analogy. A similar analogy that my chemistry professor in high school used was the following:
Think of a see-saw, if you put more weight (or increase conc.) on the left side (reactants) the see-saw, the right side of the see-saw (products) will rise. Vice Versa, if you remove weight from the left side of the equation (reactants), the left side (reactants again) will rise up.
To be honest, I like your analogy a bit better, but thought I’d give this one out if it worked better for others.
Think of a see-saw, if you put more weight (or increase conc.) on the left side (reactants) the see-saw, the right side of the see-saw (products) will rise. Vice Versa, if you remove weight from the left side of the equation (reactants), the left side (reactants again) will rise up.
To be honest, I like your analogy a bit better, but thought I’d give this one out if it worked better for others.
-
- Posts: 36
- Joined: Mon Jan 09, 2023 9:49 am
Re: helpful "Push and Pull" Analogy
Does this analogy relate to the conjugate see-saw? Since increasing [H30+] decreases [OH-]?
-
- Posts: 33
- Joined: Mon Jan 09, 2023 9:54 am
-
- Posts: 34
- Joined: Mon Jan 09, 2023 8:53 am
Re: helpful "Push and Pull" Analogy
I like to think of it as Add=Away, Remove=Toward. When something is added, the equilibrium will shift away from what was added. When something is removed, the equilibrium shifts towards it.
-
- Posts: 35
- Joined: Mon Jan 09, 2023 8:27 am
Re: helpful "Push and Pull" Analogy
Thank you, I feel like I have a better understanding of Le Chatelier's Principle when using this analogy.
Re: helpful "Push and Pull" Analogy
Could someone try explaining this in another way? I think I understand but I have trouble applying the dynamics of it in every situation; I seem only able to do it with some.
-
- Posts: 45
- Joined: Mon Jan 09, 2023 9:16 am
Re: helpful "Push and Pull" Analogy
Hi,
I'm glad that many people found this analogy useful. I have to add that this is limited to changes in concentration and partial pressure.
In the case of pressure change due to volume change (relies on a number of moles of gases on each side of the RXN) and temperature change (relies on endothermic vs exothermic reaction), this analogy would not be useful.
I'm glad that many people found this analogy useful. I have to add that this is limited to changes in concentration and partial pressure.
In the case of pressure change due to volume change (relies on a number of moles of gases on each side of the RXN) and temperature change (relies on endothermic vs exothermic reaction), this analogy would not be useful.
Return to “Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions”
Who is online
Users browsing this forum: No registered users and 9 guests