 So the first thing I'd like to do is to figure out what is the equilibrium constant expression for this reaction, okay? So why don't you guys help me out? So what is the equilibrium constant? kdq equals what? CO2 concentration of CO2 divided by what? Nothing, that's it. Okay, so that's the equilibrium constant Why? Because there's nothing over here that is aqueous or gaseous, okay? so What is the only thing that's going to be? Relevant when we're talking about the Chatelier's principle. It's part of the outside, okay? So if we increase the pressure of this reaction, right? Remember it's going to go to the side that has the least number of moles of gas Provided by the coefficients, right? So how many moles of gas does this at side that? Everybody That's not everybody And this side everyone One, okay, so which side has more? The right, the products, okay? So how about this? If I wanted to Increase the amount of products that I would get from this reaction, how would I do that? Decrease the pressure, right? So I would increase the volume of my container or decrease the put-a-backing, right? It would suck all that carbon dioxide so if I wanted to Push the reaction to the right that means increase the amount of products, right? I would increase or decrease the pressure, okay? If I wanted to push the reaction to the left, what would I do? Increase the pressure, why? Because we're squishing it down. It wants to go to the side with the least number of moles of gas. Is that okay with everybody? Yep, is that okay?