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The question gives you the standard enthalpy of formation for NO which is 90.25KJ/mole as well as a table of Absolute entropies:
N2 = 192
NO = 211
O2 = 205
The rxn is N2(g) + O2(g) -> 2NO(g) and you're asked to get delta G at 25C.
So I understand you find delta S using the given values and you multiple the enthalpy of formation for NO by 2 b/c there's 2 moles and then you plug it in to the Gibbs free energy equation but this is the answer they give:
delta G = 180.5 - (273+25)(25)(1x10^-3)
Where does the 1x10^-3 come from?
N2 = 192
NO = 211
O2 = 205
The rxn is N2(g) + O2(g) -> 2NO(g) and you're asked to get delta G at 25C.
So I understand you find delta S using the given values and you multiple the enthalpy of formation for NO by 2 b/c there's 2 moles and then you plug it in to the Gibbs free energy equation but this is the answer they give:
delta G = 180.5 - (273+25)(25)(1x10^-3)
Where does the 1x10^-3 come from?
