If a 10. m^3 volume of air (acting as an ideal gas) is at a pressure of 760 mm and a temperature of 27 degrees celsius is taken to a high altitude where the pressure is 400. mm hg and a temperature of -23 degrees celsius, what volume will it occupy? (hint: remember the temperature must be in kelvin)

15.83 m^3

Explanation:

This problem is about ideal gases.

Given that volumen, pressure and temperature, you must think about using the combined law of  gases.

This is how you solve the problem.

1) Data:

V1 = 10m^3
p1 = 760 mmHg
T1 = 27°C =  27 + 273.15 K = 300.15K

p2 = 400 mmHg
T = - 23°C = - 23 + 273.15 K = 250.15 K
V2 = ?

2) Formula

pV/T = constant =>

p1 * V1      p2 * V2
=
     T1            T2

3) Solution

=> V2 = p1 * V1 * T2 / (T1 * p2)         

V2 = 760 mmHg * 10m^3 * 250.15 K / (300.15K * 400 mmHg)

V2 = 15.83 m^3.