Why Change in Entropy for Silver, N2 & Water Similar?

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SUMMARY

The change in entropy values for 1 mol of nitrogen (N2), silver, and water (H2O) are 72.8060 J/K, 102.1817 J/K, and 86.6032 J/K respectively, with mercury also mentioned but deemed less relevant. Despite initial perceptions, these values are relatively close, aligning with textbook references. The discussion highlights the importance of understanding the thermodynamic properties of these substances to grasp why their entropy changes are similar.

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Corneo
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Can someone explain to me why the change in entropy for 1 mol of N2, silver, and water are all relatively close together? The values of the change in S I respectively are S=72.8060J/K, 102.1817J/K, 86.6032J/K, 108.8686J/K.

Yea to me they don't even look close together but they agree with the book's answer (assuming the book is correct).
 
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N2, silver and H2O are the three substances but you have four values for S
 
Opps I forgot to mention Mercury is in there also. But that's not too important. I would like to know why their delta S are all "close"
 

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