Question

The Goodyear blimps, which frequently fly over sporting events, hold approximately 1.65×105ft3 of helium.

If the gas is at 24∘C and 1.0 atm, what mass of helium is in the blimp?

Answer 1

Use the ideal gas law equation: PV=nRT
P is the pressure
V is the volume
n is the number of moles
R is the gas constant
and T is the temperature.

If the gas is at 24 C and 1.0 atm, what mass of helium is in the blimp?
--Pressure is 1 atm so we use the gas constant related to atmospheric pressure which is 0.08206 L*atm/mol*K.
--R is again 0.08206 L*atm/mol*K.
--Volume is 1.65x 105ft^3, volume must be in liters so convert 1.65 x105ft^3 into liters --n which is the moles isn't given.
--For temperature, it says the gas is at 24 Celsius and the temperature MUST be in kelvins, so 24+273.15= kelvins

Answer 2

So am I looking for the n?

Answer 3

You are looking for what mass of helium is in the blimp. n is the moles of gas, when we have the moles of gas given (after you do all the plugging in the PV=nRT equation), we calculate the mass in grams by multiplying it by molar mass of the element (helium).

Answer 4

Makes sense?

Answer 5

It's really simple, all you have to do is plug in the information you're given into the ideal gas law and after you get the moles, you multiply it by the molar mass of helium.

Answer 6

I got 62911 g. Is that right?