Textbook Problem

ou have two rigid gas cylinder. Gas cylinder A has a volume of $\text{48}.\text{2 L}$and contains ${\text{N}}_{\text{2}}\left(\text{g}\right)$at $\text{8}.\text{35}$atm at $\text{25 }°\text{C}$Gas cylinder B has a volume of $\text{22}.0\text{ L}$and contains $\text{He}\left(\text{g}\right)$at $\text{25 }°\text{C}$. When the two cylinders are connected with a valve of negligible volume and the gases are mixed, the pressure in each cylinder becomes $\text{8}.\text{71}$atm. (Assume no reaction when the gases are mixed.)

How many nitrogen molecules are present?

What is the total number of moles of ${\text{N}}_{\text{2}}\left(g\right)$mt after the gases are mixed?

What was the beginning pressure of cylinder B containing only the He(g) (i.e., before the valve urns connected)?

Think about the He(g) before and after the cylinders were connected. Graph the relationship between pressure and volume (without numbers) for the He(g) showing this change, and explain your answer, making sure to address the variables P, V, n and T.