A 28.17 g sample of liquid nitrogen (N2) starts at a temperature of -243 °C. How much energy is required to heat it to its boiling point of -196 °C and boil it completely?
S = 1.04 J/gºC delta H, = 2.79 kJ/mol

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

b is the correct answer

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