How many litres of nitrogen gas would result from spilling 3 litres of liquid nitrogen at room temperature?

a) 2049 litres

b) 365 litres

c) 3 litres

d) 800 litres

4 Answers

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  • david
    Lv 7
    1 month ago

    I don't know the density of liquid Nitrogen ...   This question is kind of screwy because the liquid Nitrogen must be at a temp of -150 deg, C (just an est.  ..  don't know it or want to look it up)  so I will use 1,0 g/ml to make a guess.

        3000 mL is about 3000 g

       3000 / 28  =  107 mol

       1 mole at STP occupies 22.4 L

       107 X 22.4  =  ~2400 L

      of your 4 choices  I would pick a 

    .. remember my numbers are just estimate so there is a lot of error 

    if the  real density is about 0.85g/ml  the calculations would be very close to  answer a.

  • Bobby
    Lv 7
    1 month ago

    V = nRT/ P

    = 86.53 mol * 293 K * 0.0820 L⋅atm⋅K−1⋅mol−1 / 1 atm 

    =  2078 L

  • Dr W
    Lv 7
    1 month ago

    room temperature is not STP billrussell42

    assuming room T = 20°C = 293K

    density Liquid N2 = 808g/L

     

    from the ideal gas law

    .. PV = nRT

    .. PV = mass / mw RT

    .. V = (mass / mw) RT/P

    then you should be able to follow

     3L.. 808g.. 1 mol .. ..0.08206 Latm/molK * 293.15K

    ---- x ------ x ----- --- x--- ----- ---- ----- ----- ----- ---- ----- = 2081 L

     1... . 1L.. .. 28.02g... .. ... .. .. 1 atm

    *********

    that doesn't match any of your choices... so YOU figure out what room temp means and update the calcs

  • 1 month ago

    density as a liquid is 0.808 g/cm³

    3 L  = 3000 mL = 3000 cm³

    0.808 g/cm³ x 3000 cm³ = 2424 g

    N₂ is 28.014 g/mol

    2424 g / 28.014 g/mol = 86.53 mol

    One mole of any ideal gas at STP has a volume of 22.41L

      (old def of STP, 1 atm)

    22.41 L/mol x 86.53 mol = 1939 L

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