 Okay, so this is a good one, I think. This goes over Le Chatelier's principle and it asks which way will the reaction shift or the equilibrium shift if the temperature is increased? So in order to know which way the reaction will shift for this one, you've got to make understand whether it's an exothermic or endothermic reaction. So it's got a negative charge from the delta H, right? That means that it's an exothermic reaction. And it also means that heat is a product of the reaction. Okay, so heat is the product, so you can put heat over there. So if you increase the temperature, that means you're increasing heat. Okay, now when you increase the product, right, since heat's a product, it's going to push the reaction back to the left or towards the reactants. So your reaction arrow will look something like this. Or the big arrow is being pushed towards the reactants. If the pressure is increased, okay, so that's like if you have a piston, right, and you push that piston down, that increases the pressure. But if you do that, the number of moles of gas wants to get smaller, okay? So if you look here, you've got two moles of gas here and two moles of gas here. So in actuality this isn't a very good problem to do this one on because it doesn't show anything because increasing the pressure or decreasing the pressure doesn't change the number of moles of gas. So there would be no shift here because when you increase the pressure, you want to decrease the number of moles of gas, but since there's two moles on the reactants and two moles on the product side, it doesn't matter which way you go, they're both two moles. And the catalyst is added, this will never change. It just speeds up the reaction. Yeah, it just speeds up the reaction. It just changes the thermodynamics of the reaction. It doesn't change the kinetics of the reaction at all. It doesn't change the equilibrium of the reaction. It only changes the kinetics of the reaction. So in other words, there is no shift here. So I wish we would have done one where there was a shift on one of the...