chemistry question I dont get

Question

Typically, when a person coughs, he or she first inhales about 2.00 L of air at 1.00 bar and 25 ∘C. The epiglottis and the vocal cords then shut, trapping the air in the lungs, where it is warmed to 37 ∘C and compressed to a volume of about 1.70 L by the action of the diaphragm and chest muscles. The sudden opening of the epiglottis and vocal cords releases this air explosively. Just prior to this release, what is the approximate pressure of the gas inside the lungs?

Express your answer numerically in bars.

please help I do not get this show all the work please I'm confuse

Answer 1

Combined gas law: P1V1/T1 = P2V2/T2

P1 = initial pressure = 1.00 bar

V1 = initial volume = 2.00 L

T1 = initial temperature in K = 25º + 273 = 298K

P2 = final pressure = ?

V2 = final volume = 1.70 L

T2 = final temperature = 37º + 273 = 310K

Solving for P2, we have...

P2 = P1V1T2 / T1V2 = (1.00)(2.00)(310) / (298)(1.70)

P2 = 1.22 bar