Nitrogen gas is stored in a 0.3 m3 tank at 700 kPa and 25oC. Gas is allowed to f

Question

Nitrogen gas is stored in a 0.3 m3 tank at 700 kPa and 25oC. Gas is allowed to flow from the tank through a partially opened valve into a gas holder that has a constant pressure of 80 kPa. Assume that nitrogen is an ideal gas for which y = 1.4. When the pressure in the tank has dropped to 300 kPa, calculate the mass of nitrogen in the gas holder if the process takes place slowly enough that the temperature in the original tank can be held constant.

Nitrogen gas is stored in a 0.3 m3 tank at 700 kPa and 25°C. Gas is allowed to flow from the tank through a partially opened valve into a gas holder that has a constant pressure of 80 kPa. Assume that nitrogen is an ideal gas for which 1.4, when the pressure in the tank has dropped to 300 kPa, calculate the mass of nitrogen in the gas holder if the process takes place slowly enough that the temperature in the original tank can be held constant.

Explanation / Answer

Nitrogen being an ideal gas, follows ideal gas equation.

For the original tank, volume and temp=const

Thus, P1n1 = P2n2

Initially, PV= nRT

(700 x 1000 Pa) x (0.3 m3 ) = n1 x 8.314 J/mol-k x 298 K

Thus, n1 = 84.76 moles

After the pressure drop,

n2 = P2/P1 x n1 = 3/7 x 84.76 = 36.326 moles

Moles lost = moles gone to gas holder = 48.434 moles

Mass in gas holder = 48.434 moles x 28 g/mol

= 1356.156 g

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