Have you guys heard of citric acid before? Yeah, I've heard of it too. Yeah, it's in like every single soda. It's a food reserve. It's in citrus fruits. Let's go more. A lot more. Yeah, it's like triple that. Look how big the jar is. Yeah. Yeah, I know. Always scoop relative to the size of the jar you have. Yeah. OK. And let's put about an evil amount. And let's wipe that sucker out. Because it's this. And let's put about an evil amount of baking soda in. So we just go to our manhammer sodium bicarbonate. Because it's an alpha-cellsir. Yeah, it's alchacelic acid has baking soda. And usually tartric acid. Oh my god. It is. Well, so in this reaction, yeah, that's going to be more. So in this reaction, we're saying we make a guess. So we're trying to seal this sucker up here. Let me see if I can just remove this piece. Usually we don't want these to come off. You want to do it? Yeah. All right, we're going to pour. So I'm going to ask you to pour carefully into this little hole here. Carefully. Go for it. I'll tell you when. OK, that's probably good. So we're going to seal this up. Go ahead and do it a shake. And feel the bottom. Tell us that you think it's getting hotter. It's like foam. And the air is like foam. The foam up there. The foam up there. So we definitely see all the bubbles forming right, which we know is which one. Is it going to pop? It's going to pop. No, it's going to pop. It's going to pop. It's going to pop. It's going to pop. It's going to pop. It's going to pop. I'm going to see that. I'm going to see that. I'm going to see that. So yeah, so we made a lot of carbon dioxide, right? And yeah, what do you say is hotter foam? It's really cool. It's really cool to go on a hand out around again for people to feel. Well, I won't end with this again. So we definitely formed the gas right that we're saying according to our equation here. And so my delta H value is, is that going to be positive? Once like once, because we're seeing for this reaction, the absorb heat or release heat. So it's going to absorb heat. It's cold, right? The absorb heat is cold, which was end of the micro-exothermic end of, which is in its endothormic end of the absorb heat, cool, and people in the reaction. So then my delta H is that positive or negative? What did you say over here? Yeah, we absorb heat, right? We absorb heat. It's endothormic. It's a positive value. So here my endothormic is a awesome positive value, positive, whatever. I'm not sure exactly. Positive, whatever. So now if I look at, oh, sorry. And lastly, was this favorable or unfavorable? This is unfavorable. Right? It is, I had to absorb, I had to absorb energy in order to feel that that was cold, right? Yeah, it is. It was cold because it was absorbing heat from your hand. That's how you feel cold, right? You can be transferred heat to something. So definitely, that was a cold reaction, absorb heat. Now I have my two terms. According to enthalpy, this reaction shouldn't happen. According to entropy, it shouldn't happen. Which seemed like you're going at odds, right? But using our observations, what do we know that delta G must be? So the data is positive. Positive, positive. Two positives make that positive. Well, it's going to be equation. Delta G equals delta A minus T delta S. We said delta A is a positive value, right? Delta T S is a negative. Sorry, it is also positive. So here I have a positive number minus some number. But this number can change sizes, depending on the temperature, right? What have a positive number? And I'm subtracting something? If it's small, it's going to stay positive. But it is really big, and it's going to be negative, right? So what does that mean? It's going to be negative. That S is probably really big, or the temperature is really big. One of these terms is bigger than the enthalpy term. So we'd say that this is intropically driven, and tropically driven. The entropy is always more important. Intropically driven, the delta H, the T delta H, the T delta S, excuse me, factor is large. So we have a big difference in entropy, and that's bigger than the changes in the bond energies. Because what did we observe? We know that delta G has to be what? Because we saw the reaction occur. It has to be negative, we saw it occur. It occurred, it was favorable. If I make all this things together, nothing happened, then maybe it's positive. Well, according to your chemical reaction,