Question

Le chateliers principle question

Answer 1

he stated that when a chemical systems equilibrium is is disturbed, the system always appears to react in direction that opposes the change until new equilibrium


what does that mean? example?

Answer 2

Ok we'll uses a simple reaction to explain I like to use 2h2 + o2 <-> 2h2o

Answer 3

If we add either of the reactants(h2 or o2) the reaction will try to rebalance itself but making more product until equilibrium is reached

Answer 4

One the other hand if h2o is added the reaction will shift in the direction of the reactants until equilibrium is reached

Answer 5

Additionally if pressure were to increase(decrease in volume) the reaction will shift to the side with less moles which is the product side 3 vs 2 mols and visa versa is pressure were to decrease the reaction will shill to the side with more moles the left side (reactants)

Answer 6

I hope this helps

Answer 7

ok makes sense now! one more question, when you add or remove energy so endo or exo

which one is producing products and which reactants?

Answer 8

my text book is kinda confusing as it contradicts itself.... @zoomiemoo

Answer 9

This confused me too I thought I was never going to get it

Answer 10

when you think about it exothermic reactions make energy energy a->b+heat. If you add heat the reaction will try to counteract it by shifting to the reactants so not as much heat is lost in the first place

Answer 11

does that make sense?

Answer 12

ok so that's what I thought, but for one example.....

Answer 13

it said it shifted right so more products favoured but that didnt make sense....