How do you know when the equilibrium has shifted when the temperature of the potassium nitrate is lowered?

Question

I know that the equilibrium moves towards the reactants or the products that absorb the heat... I think. This might have something to do with the question

Answer 1

I suspect that the questioner is talking about the solubility curve of potassium nitrate. KNO3 dissolves endothermically. If you increase the temperature, more dissolves to try and "take in" the extra heat.
Conversely, if you cool a saturated solution, you will see crystals forming, because the equilibrium is trying to release heat.

Answer 2

In an exothermic reaction, a decrease in temperature causes a shift to the right.

In an endothermic reaction, a decrease in temperature causes a shift to the left.

Answer 3

i think of you could examine it with a pH meter (and then making the calculations of path) , or you could think of roughly it with the Le Chatelier theory. Rmember that temperature impacts the equilibrium consistent, so which you will set off it, or verify it with a pH meter. or verify the products.