In real life, a given system can approach equilibrium from different starting points but will still have the same equilibrium constant. How is this possible?

Question

anonymous · Answer

@Tazmaniadevil

anonymous · Answer

At a given temperature a given reaction will have a k value (equilibrium constant), and this will stay constant. What this means is that the amount of product you will make will change because the k value cannot. 

For example you have a reaction that has reached equilibrium, but you decide to add more of whatever you're products were, you're equilibrium will shift to make more reactant.

This is what is known as La Shatliere's principle (there is no way that's spelled right). The reasoning behind this involves a lot of thermodynamics and kinetics knowledge, but this is a start

anonymous · Answer

Wow! the intelligence you posess is overwhelming. Thank you so much! that makes way more sense than the answers people had given me before. Ah! Thank you thank you!!!

anonymous · Answer

your welcome hun i try my best for the best for yall as would u try the best for ur friends and u are a good friend so i will do my best for you

anonymous · Answer

Thank you! if you ever need help i will do my best!

anonymous · Answer

;)

anonymous · Answer

you need anything else

anonymous · Answer

nope thats the last thing i needed for today :)

anonymous · Answer

sweet good luck

somy · Answer

@tazmaniadevil 
Le Chatelier's principle
lol