 Okay. Okay. So if the equilibrium constant is 0.123, calculate the concentration of ammonia. If the concentration of nitrogen is 0.058 molar and the concentration of hydrogen is 1.24 molar. Okay, so first you need to know how to figure out what the equilibrium constant is. So, and in this part, in this problem you would have done that in part A anyways, right? So KBQ equals the concentration of ammonia squared over the concentration of nitrogen times the concentration of hydrogen Q. So it gives you these values for KBQ H2 and N2 and it asks you to figure out what NH3 is, right? So what you need to do is isolate that variable NH3, okay, the concentration of ammonia. So in order to do that, you're going to put everything else onto the other side of the equation, okay? So you're going to take both sides of this equation, multiply by concentration of N2, cancel N2 out there, then you'll multiply it by H2Q, concentration of H2Q. And that'll cancel it there. But we'll write, let's write what we got now. So we've got concentration of the NH3 squared equals the concentration of H2Q times the KBQ. So that in order to get rid of a square, you take the square root of both sides, right? So we take the square root here, that cancels with that, and we take the square root there. Okay. So our new equation is this. The concentration of ammonia equals the square root of H2Q times N2 times KBQ. We'll just plug this in. So H2 cubed, 1.24 cubed times N2, 0.508 times KBQ, 0.123. And then put it on your couple of units because this equation is not going to give you the right units if you try to plug them in. So you've got to remember that when the brackets are around something, it's the molar concentration.