 So let's try this one Equilibrium constant problem. It says consider the following equilibrium process at 700 degrees Celsius, and then it shows the chemical equation Analysis shows that there are 2.50 moles of hydrogen 1.3 times 10 to the negative fifth moles of sulfur and 8.70 moles of hydrogen sulfide present in a 12 liter flask Calculate the equilibrium constant for the reaction. Okay, so it wants us to actually calculate Kc so Let's write down the Kc expression first So Kc is going to be of course the products to their coefficients divided by the reactants to their coefficients, right? Okay, so concentration H2s squared divided by the concentration of H2 squared times the concentration of S2 Okay, why why do we use them all because they're all gasses? Okay, so If you notice they're brackets, right? So that means concentration in molarity. Okay, so if we look over here, right? We've got moles That's not molarity. Okay, but we've got a volume here so we can convert all of these to molarity. So let's do that first so 12.0 liters 12.0 liters 0.208 Molver 2 times 10 to the negative 6 8.7 So now all we do is plug and chug On the top And remember in this we don't put our units because Kc doesn't have any units Okay Okay, what did you get as an answer? 1.08 times 10 to the Sorry, what'd you say? 1.08 times 10 to the 7th block Is that what it says? Yeah Just like you said So any questions on that one? No. Okay. Yeah, so I had my formula set up right that Kc goes to my product over the reaction. Uh-huh. It just died. I messed up with the The actual punching the numbers into the calculator. Yeah, okay So I guess the main point is in these ones to remember since it says Kc You got to convert it to molarity and then don't put your units in your Kc. Okay