In the following example question it says when this reaction comes to an equilibrium, which will be higher in pressure reactants or products. So here we have two moles of chapter 4 reacting with two moles of H2S to produce. We have here CS2 and H2. We're told that our equilibrium constant in the form of KP is 1.3×103.
Here we can see that K is greater than one. Remember when K is greater than one, we say that the product side is favored and the forward direction is favored. So the side that's favorite are our products, which means we're making more of them. And when it comes to the pressure of gases, the more particles or molecules of gases present, the higher the pressure.
Since we have more products being favored, they would have an overall greater pressure. This would mean that out of all of our options, option B is the correct choice. Product side is favored. There's more products, therefore they will result in higher pressure.