The following diagram represents a reaction shown going to completion. Each molecule in the diagram represents 0.1 mol, and the volume of the box is 1.0 L. (d) Assuming that all of the molecules are in the gas phase, calculate n, the change in the number of gas molecules that accompanies the reaction. [Section 15.2]

Video transcript

Hello everyone today. We have the following problem. Consider the following diagram of a gas phase reaction. Whereas each molecule represents one mole in a box with a volume of one leader. What does it change the number of gas molecules as a result of the reaction? So we have a box on the left here in the box on the right for the first box we see that we have five molecules of X Gas. We have seven molecules of Why gas. In the second box we have four molecules of XY two gas and we also have one excess of x gas and one excess of gas. So this tells us that our reaction is going to be four X gas molecules reacted with six y gas molecules to form four X molecules As well as why three molecules. and so simplified simply dividing this entire both sides by two. We get two x molecules plus three y molecules to give us two x molecules as well as to why wallet kills. And so our change in N is going to essentially be products minus our reactions. And so our products, we have two moles And for our reactant we have five moles. And so our change and N is going to be negative three. Giving us our final answer. I hope this helped. And until next time