 So let's try this one. We're going to compare q and k to determine the reaction direction this time For the reaction that's pictured on the board At what point during the reaction Does the concentration of N2O4 equal 0.12 molar and the concentration of nitrogen dioxide equal 0.55 molar So let's figure that out. Let's figure out what qc is at that point in time. Okay, that's what it's asking So how do we do qc first thing? We got to figure out. Well, what is qc? So, yes, yes, so both of them are going to be in it. N02 squared divided by concentration of N2O4 like that So remember qc no unit, so it doesn't matter if you put your molarity in here or not So I'm just not going to do it just for a change Okay, so at the top I'm going to put 0.55 And square that And at the bottom 0.1. So when I do this 0.55 squared divided by 0.12 I get well the two six is 2.5 Okay, so 2.5 is qc Is that equivalent to 0.21 2.5? No clearly not so it's bigger than it right so let's write that down So qc is greater than kc Does that make sense everyone? greater than kc So is this reaction at equilibrium? That's one of the things it's asking us. No, it's not at equilibrium Why is that? Because if it were at equilibrium, what would happen? q and k would be equal right? Then the next thing it asks us well since it's not which direction is it progressing as it progressing towards products or towards reactants Towards reactants right so q is bigger than c then it's going back towards reactants pretty good