A tank that is 0.500 m^3 in volume has 21.6 liters of liquid nitrogen in it. The liquid nitrogen is at its boiling point of -196°C. (Possibly useful information: density of liquid nitrogen (N2), 808.4 kg/m3; latent heat of vaporization of liquid N2(N subscript 2), 1.99 x 10^5 J/kg; specific heat of liquid N2, 1.04 x 10^3 J/(kg·°C); specific heat of gaseous N2, 2.04 x 10^3 J/(kg·°C))
a) What is the mass (in kg) of liquid N2 in the tank?
b) 7.00 MJ (7.00 x 10^6 J) of heat is added to the liquid nitrogen. How much nitrogen is converted to a gas, and what is its final temperature (in °C)? Assume that it starts entirely as a liquid.
c) The molecular weight of N2 is 28.01 grams per mole. Find the pressure inside the 0.500 m^3 tank (in atmospheres) after adding the 7 MJ of heat.
d) A youtube video shows an ABS plastic pipe bursting at a pressure of 455 psi. If we put the 21.6L of liquid nitrogen in a pipe with a volume of 0.500 m^3, seal it, and let it come to room temperature (22°C), will it burst? If not, how much additional pressure is necessary? Show your calculations.