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?

Question

Chemistry

Brooke Villarreal

13 May, 18:26

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?

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Deacon Hanna · Answer 1

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