I was wondering if my answers are correct. I am a bit confused about how to know what colour the reaction will turn into
Hey! From your answers, I think you've got the right idea with the colours. Basically, if the equilibrium favours the forward reaction, the concentration of the products on the right will increase and thus their colour will become more prominent, vice versa
Q2 first photo- for the concentration of Cl
- to increase, it will shift left
Q3 first photo- this is an exothermic reaction, meaning that heat is
released. So when temperature is decreased, equilibrium will favour the
exothermic reaction to produce more heat, which is the forward reaction in this case. Does that make sense?
Same goes for Q4 on the same photo, except this time it will favour the backward endothermic reaction since temperature is increased
Q5 first photo- you're right that OH
- will react with H
+ to form water! This reduces the concentration of H
+. As a result, equilibrium will shift left to oppose the change and produce more H
+I'll have a look at the second photo and edit this post in a bit! Unless someone beats me to it haha.
Edit: ok I'm back!
Q3 second photo- there is actually
no change to equilibrium here. Remember that the three factors affecting equilibrium are concentration, temperature and pressure. By removing
solid iodine, its concentration/density isn't affected! Therefore, there will be no shift. Same goes for adding a solid. Good to note that
Le Chatelier's Principle does not apply to solidsQ4 second photo- pressure will only affect gases in equilibrium. So because iodine is in solid form on the right, the mole ratio of gases is actually 1:0. Therefore, when volume is increased, pressure decreases, so equilibrium will shift to the reaction which produces
more moles of gas, ie the backward reaction
Q5 second photo- same with 3&4 of the first photo, the equilibrium will shift to favour the backward endothermic reaction to reduce the temperature
Hope this helps
Let me know if anything doesn't make sense!