Starting with 21.5 moles of O2 in a bottle, calculate the volume of O2 the bottle could deliver to a climber at an altitude where the temperature is –38.0°C and the atmospheric pressure is 0.402 atm.

Question

Starting with 21.5 moles of O₂ in a bottle, calculate the volume of O₂ the bottle could deliver to a climber at an altitude where the temperature is –38.0°C and the atmospheric pressure is 0.402 atm.

answer in Liters

Answer 1

21.5 moles of O₂ = n

38.0ºC + 273 = 311K = T (temperature)

0.402 atm = P (pressure)

R = gas constant = 0.0821 L-atm/K-mol

Ideal gas law:

PV = nRT and solving for V (volume)...

V = nRT/P = (21.5 moles)(0.0821 Latm/Kmol)(311K)/0.402 atm

V = 1366 liters of O₂ = 1370 liters (to 3 significant figures)