- #1

molly16

- 16

- 0

N2O4:

gibbs energy of formation = 99.8 kJ/mol

Enthalpy of formation =11.1 kJ/mol

Entropy = 304.3 J/mol K

NO2 :

gibbs energy of formation = 51.3 kJ/mol

enthalpy of formation = 33.2 kJ/mol

entropy = 240.1 J/mol K

N2O4 (g) <=> 2NO2 (g)

Attempt at a solution:

So first I found the enthalpy and free energies of the reaction

delta Hrxn = 2(33.2) - 11.1 = 55.3 kJ/mol

delta Grxn = 2(51.3) - 99.8 = 2.8 kJ/mol

since the surroundings are at constant pressure I know:

delta Ssurroundings = qsurroundigs/T = delta H surroundings/ T

but I'm not sure where to go from here. Can anyone help?