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Given that standard enthalpy of formation for NO(g) is 90.25 kJ/mole, calculate the free energy of the rxn:
N2 + O2 ------> 2NO
N2 = 192, NO = 211, O2 = 205 (all in J/mol.K)
Answer: 180.5 - (298)(25)(1 x 10^-3).
Is this a mistake? I thought it should be 1 x 10^3.
N2 + O2 ------> 2NO
N2 = 192, NO = 211, O2 = 205 (all in J/mol.K)
Answer: 180.5 - (298)(25)(1 x 10^-3).
Is this a mistake? I thought it should be 1 x 10^3.
