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This is a followup to my previous post: thanks for the advice on the two questions. I got the HH one. That was quite easy.

However, I'm not getting this one correctly:

N2O4 --> 2NO2

Delta G is 2.8kJ (under standard conditions). At what temp will it become spontaneous?

So. I know Gibb's is: Delta G = Delta H - T(delta S)

The delta H for N2O4 is 9.66 and NO2 is 33.85

The delta S for N2O4 is 304.3 and NO2 is 240.46

This is per my book

I plug those into the Delta H and Delta S equations:

2(33.85) - 9.66 = 58

2(240.46) - 304.3 = 176.9

T = Delta H / Delta S

This comes out to 0.328 K

That can't be right! What did I do wrong?

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