Question

a balloon is blown up to a pressure of 1.50 atm at a temperature of 40 degrees celcius. Tests show that the balloon contains exactly .250 mole of air. What is the volume of air in the balloon

Answer 1

To solve this problem we assume that air inside the ballon behaves as an ideal gas, for which we can describe such behavior with the ideal gas law:

PV = nRT

Where P stands for Pressure, V for volume of the substance, n are the moles, R is the universal gas constant (0.082 Latm / Kmol), and T for temperature in Kelvin.

We have pressure, temperature, and moles, from which we can obtain volume:

PV = nRT

1.5 atm * V = 0.25 moles * 0.082 L atm / K mol * (40C + 273.15)

V = 6.4196 L atm / 1.5 atm = 4.28 L = V