Ideal Gas law Problem

Question

2. After the child has exhaled all of this gas, it becomes sick. If its temperature rises to 42.0 C and it can hold 0.150 moles of air in its lungs at a pressure of 1.15 atm, what is the new volume of the child’s lungs?
3. 
   

Answer 1

Hello, Emily,

We'll use the ideal gas law, with a gas constant of R = 0.08206 L*atm/K*mol, since it has the same units as the data provided.

PV = nRT, rearrange for the unknown, V:

V = nRT/P

V = (0.15 mole)*(0.08206 L*atm/K*mol)*(315.15K)/(1.15atm)

Make sure the units cancel to leave just the volume:

V = (0.15 mole)*(0.08206 L*atm/K*mol)*(315.15K)/(1.15atm)

V = 3.37 liters

Bob