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?

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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

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