# What is the volume of 6 moles of helium gas at 0.34 atm pressure and 33°C and what is the density of the helium gas under these conditions? The volume of an ideal gas is dependent on the amount of the gas, the temperature and the pressure. The ideal gas law is: PV = nRT, which gives V = n*R*T/P where n is the number of moles, T is the temperature in Kelvin, P is the pressure and...

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The volume of an ideal gas is dependent on the amount of the gas, the temperature and the pressure. The ideal gas law is: PV = nRT, which gives V = n*R*T/P where n is the number of moles, T is the temperature in Kelvin, P is the pressure and R is a constant equal to 8.205746*10^-5
m^3*atm/K*mol

Here, the number of moles n = 6, the pressure is 0.34 atm., the temperature is 306.15 K.

The volume is V = 6*8.205*10^-5*306.15/0.34 = 0.4432 m^3

The volume of the gas is 0.4432 m^3. The molar mass of Helium is 4, 6 moles of helium weighs 24 g.

This gives density as 24/0.4432 = 54.14 g/m^3