Ok, so using Le Chatelier's Principle
If you add heat to an exothermic reaction, the equilibrium will shift to the left.
If you remove heat to an exothermic reaction, the equilibrium will shift to the right.
What is it for an ENDOTHERMIC reaction?
If you add a substance, the equilibrium will shift to the other side.
If you remove a substance, the equilibrium will shift to the same side.
If you increase pressure/decrease volume, then the equilibrium will shift to the side with the less moles.
If you increase volume/decrease pressure, then the equilibrium will shift to the side with more moles.
Please tell me if this is right, thank you :)
All of those are right. For the endothermic rxn (or exothermic) look at it this way and it will make a lot of sense.
A + B ==> C + heat for exothermic so adding heat works just like adding a reagent; i.e., adding A or B shifts to the right. Adding C shifts to the left. Adding heat shifts to the left.
Endothermic rxn.
A + B + heat ==> C
Adding A or B or heat shifts to the right. Adding C shifts to the left.
Thank you Dr. Bob
Yes, you have correctly described the effects of different factors on the equilibrium of both exothermic and endothermic reactions using Le Chatelier's Principle!
For an endothermic reaction, the equilibrium can be shifted by adding or removing heat, just like in an exothermic reaction. However, the effects on the equilibrium are opposite.
- If you add heat to an endothermic reaction, the equilibrium will shift to the right, favoring the products. This is because the reaction absorbs heat, so adding more heat promotes the forward reaction to consume the additional energy.
- If you remove heat from an endothermic reaction, the equilibrium will shift to the left, favoring the reactants. This is because the reaction requires heat and removing it causes the reverse reaction to occur, generating more heat to compensate.
Regarding the effect of adding or removing substances:
- Adding a substance (reactant or product) to a reaction will cause the equilibrium to shift to the opposite side, regardless of whether it is endothermic or exothermic. This is because increasing the concentration of one species will cause the equilibrium to shift in the direction that consumes or generates more of that substance, in order to restore equilibrium.
- Removing a substance will cause the equilibrium to shift in the same direction as the substance has been removed, regardless of whether it is endothermic or exothermic. This is because reducing the concentration of one species will cause the equilibrium to shift in the direction that replaces or consumes less of that substance, in order to restore equilibrium.
Lastly, regarding the effect of changes in pressure/volume:
- Since pressure is directly proportional to the number of moles, increasing pressure or decreasing volume will cause the equilibrium to shift towards the side with fewer moles of gas. Similarly, decreasing pressure or increasing volume will cause the equilibrium to shift towards the side with more moles of gas. This principle applies to both endothermic and exothermic reactions.
Overall, your understanding of Le Chatelier's Principle seems to be accurate! Keep in mind that the mentioned factors only describe the immediate response of the equilibrium system, and the final equilibrium position may involve multiple factors simultaneously.