 OK, so this problem says, for the synthesis of ammonia, the equilibrium constant, so Kc, at 375 degrees Celsius is 1.2, and we have that written up there. Starting with an initial concentration of hydrogen of 0.76 molar, nitrogen at 0.60 molar, and ammonia at 0.48 molar, which gases will have increased in concentration and which gases will have decreased in concentration when the mixture comes to equilibrium. So you might think, at first glance, that you're going to need to do a nice table for this one, but you actually don't. What you need to do is compare Q and C. So let's write our Q and K, sorry. So let's write what Qc would be. So it would be the same expression as Kc, right? So concentration of ammonia squared divided by nitrogen times the concentration of hydrogen Q. So it gives us these initial concentrations. So what we want to do is just plug those in directly. So divided by nitrogen at 0.60, hydrogen at 0.76. Let's figure out what that is equal to. So the number I got was 0.87. So if we look, right, Q and Qc and Kc, if we're going to compare them, what we find is that Kc is bigger than Qc. So in this case, whenever Q is smaller than K, that means the reaction has to go to the right to get to equilibrium. So it still needs to go to the right. So the question asks us which concentrations would increase and which concentrations would decrease, right? So as the reaction goes to completion, if we're going to the right, the concentration of hydrogen gas is going to decrease, the concentration of nitrogen gas is going to decrease, and the concentration of ammonia is going to increase. So it's effectively like telling you how to do your ice table to say minus, minus in the reactants and plus in the products, OK? That's all you've got to do for this one. Any questions on that one? No. OK. Is it easy? Yeah, it's much easier than what you would expect. The problem is, is that you know about ice tables already, so you can't kill it.