What volume of N2 is released at 0.930 atm of pressure and 25.0°C from a tank of liquid N2 (d = 0.808 g/mL)?

This is an incomplete question, here is a complete question.

Students at the University of North Texas and the University of Washington built a car propelled by compressed nitrogen gas. The gas was obtained by boiling liquid nitrogen stored in a 200.0 L tank. What volume of N₂ is released at 0.930 atm of pressure and 25.0 degrees Celsius from a tank full of liquid N₂ (d = 0.808 g/mL)?

Answer : The volume of N₂ released is,

Explanation :

First we have to calculate the density of N₂ in 200.0 L volume.

Conversion used : (1 L = 1000 mL or, 1 mL = 0.001 L)

As, density of N₂ in 1 mL = 0.808 g

So, density of N₂ in 1000 mL = 1000 × 0.808 = 808 g/L

Now we have to calculate the mass of N₂

Now we have to calculate the volume of N₂ released.

Using ideal gas equation:

where,

P = pressure of gas = 0.930 atm

V = volume of gas = ?

T = temperature of gas =

R = gas constant = 0.0821 L.atm/mole.K

w = mass of gas = 161600 g

M = molar mass of N₂ gas = 28 g/mole

Now put all the given values in the ideal gas equation, we get:

Therefore, the volume of N₂ released is,

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