A large weather balloon requires plenty of helium gas in order to ascend into the atmosphere to take measurements. If the balloon has a volume of 100,000 liters, about how many moles of helium gas would be required to fill the balloon to a pressure of 1 atm and a temperature of 27 degrees C?
To be able to calculate the number of moles for this problem, for simplicity, we assume that it is an ideal gas. We use the equation PV = nRT. We do as follows:
PV = nRT n = PV / RT n = 1(100000) / 0.08206 (27 + 273.15) n = 4060.04 mol
