A balloon holds 31.6 kg of helium. What is the volume of the balloon if the final pressure is 1.2 atm and

. . . the temperature is 22°C?

It's on my WebAssign and I can't figure it out. Thank you!

Ideal Gas Law: PV = nRT

P = pressure (atm)
V = volume (L)
n = number of moles (mol)
R = gas law constant = 0.0821 L*atm/mol*K
T = temperature (K)

***Temperature MUST BE IN KELVIN.***

1. Convert 31.6 kg He -> mol He

Kg -> mol

Given kg x 1000 g/1 kg x 1 mol/molar mass

31.6 kg He x 1000 g He/1 kg He x 1 mol He/4.003 g He = 7894.1 mol He


2. Convert 22°C -> K

°C -> K

Given °C + 273 = K

22°C + 273 = 295 K


Plug everything in:

1.2L = 7894.1 x 0.0821 x 295
1.2 L = 191191.2
L = 159325.97 L


Sig figs... 160000 L

umm sorry this is more of a question
err im not that clever or even a bit clever but how does one weigh something that is lighter than air???
im not trolling i realy want to know .

That's more like a small airship than a balloon. It would take a lot of helium to weigh 31.6kg.