Pure N2 at 25°, 100 kPa is slowly heated in a cylinder fitted with a piston. The cylinder has stops at one end such that when the piston is fully extended the volume is 10 times the original volume. You may assume ideal gas behavior and neglect ionization. Natural logarithms (base e) of the equilibrium constants for Nitrogen dissociation are: T (°K) In KT In KT N₂ = 2N NN + e 4000 -12.66 -23.87 4500 -9.41 -22.17 5000 -6.81 -18.94 5500 -4.67 -17.41 6000 -2.87 -11.91 a. At what temperature would the equilibrium composition contain 1% by mass of monatomic N? b. Is the ideal gas assumption justified? c. Is it reasonable to neglect ionization?