Question

A cylinder with a movable piston originally has a volume of 2805 mL and is filled with nitrogen to a pressure of 4.00
atm. The piston is then allowed to move outward until the volume of the cylinder is 3864 mL. What is the pressure
of nitrogen in atm in the cylinder at this point? The temperature of the cylinder remains constant at -5°C. Your
answer must have the correct number of sig figs. P =
atm

Answer 1

This problem is providing the initial volume and pressure of nitrogen in a piston-cylinder system and asks for the final pressure it will have when the volume increases. At the end, the answer turns out to be 2.90 atm.

Boyle's law

In chemistry, gas laws are used so as to understand the volume-pressure-temperature-moles behavior in ideal gases and relate different pairs of variables.

In this case, we focus on the Boyle's law as an inversely proportional relationship between both pressure and volume at constant both temperature and moles:

$P_1V_1=P_2V_2$

Thus, we solve for the final pressure by dividing both sides by V2:

$P_2=\frac{P_1V_1}{V_2}$

Hence, we plug in both the initial pressure and volume and final volume in order to calculate the final pressure:

$P_2=\frac{2805mL*4.00atm}{3864mL}\\ \\P_2=2.90atm$

Learn more about ideal gases: brainly.com/question/8711877