You can use the ideal gas law to find the volume:
PV = nRT
V = nRT/P (use R=0.08206 L*atm/mol*K)
= (4.0 mol)*(0.08206 L*atm/mol*K)*(300K)/(2.0 atm)
V = 49.24 L
450k
5.64 ATM
Since PV=nRT, increasing the pressure 6 fold will decrease the volume to 1/6, assuming temperature is constant, thus the volume becomes 0.4 L
3.0 atm
First let's convert 204.6kPa to atm: 204.6 / 101.3 = 2.02atm. Now, use PV = nRT: (2.02)(V) = (0.80)(0.0821)(300), solve for V to get 9.75L, so a 10L container would work just fine.
0.77
(32.0 g/46.0 g/mol) (0.0821 atm) (291.0 K) / 3.12 atm
PV = nRTV = nRT/P = (2.00 mol)(0.08206 Latm/kmol)(573K)/(2.62 atm)V = 35.9 liters (to 3 sig. figs.)
125 mol.
PV = nRTV = nRT/P = (2.00 mol)(0.08206 Latm/kmol)(573K)/(2.62 atm)V = 35.9 liters (to 3 sig. figs.)
19.48
5.64 ATM
The volume is 13,64 L.
Since PV=nRT, increasing the pressure 6 fold will decrease the volume to 1/6, assuming temperature is constant, thus the volume becomes 0.4 L
3.0 atm
38 L
38 L
Carbon dioxide Argon Oxygen Helium Nitrogen