Now let's take a look at the effect that temperature has on our equilibrium status, based on the Schotteler's principle. Here we're going to say changing the temperature of the reaction at equilibrium will disrupt the equilibrium and cause a shift. But how exactly does it work? Well, we're going to have to say here that enthalpy, which remembers ΔH of a reaction, plays a big role in the direction of the change.
Here we're going to say, recall that the equilibrium constant is temperature dependent. So changing the temperature not only can affect which way we shift, but it can also affect the scale or value of your equilibrium constant K. So here, let's take a look. We have enthalpy type. We have the type of change that can occur whether we're increasing or decreasing. We have examples and then we have explanations.
So in the first row, we have the explanation that we're shifting away from heat. Now we shift away from heat if we're increasing the temperature. Now this is true whether it's exothermic or endothermic. Increase in the temperature causes the shift away from the heat source. If we're talking about an exothermic process, ΔH is negatively charged. Exothermic means we're releasing heat. So heat has to be a product.
All right. So we increase the temperature, we're going to shift away from the heat, which means I'd have to move away from it. So I'm going to move towards the reactant side. We're going to go to the left. Remember the direction you shift in that side would be increasing an amount, so our reactants would increase in amount and conversely the product should be decreasing out. Because remember if one side is increasing, the other side has to be decreasing.
Now here for the 2nd row, we're shifting towards the heat. Now this is true whether it's endothermic or exothermic. If we decrease our overall temperature of the chemical reaction, the reaction have to shift towards the heat. So here, if you're an endothermic process, your enthalpy is pop. Your enthalpy is positive. If it's positive, you're absorbing heat, so he has to be a reactant. We are decreasing our temperature, so we're going to shift towards it. In this case, we're moving towards the left, again towards the heat. So again, wherever you're moving to, we'll be increasing an amount. If this side is increasing, the other side is decreasing.
So when it comes to this idea of temperature, Le Chatelas principle, first it's important to understand is your reaction endothermic or exothermic? This will tell you what side heat will be found. Once you've established a location of heat, then you look to see OK, is my heat, is my temperature increasing or decreasing? If temperature is increasing, I shift away from the heat. If temperature is decreasing, I shift towards the heat. So keep that in mind anytime you're dealing with a question that ties together temperature and Le Chatelier's principle.