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,

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.