Molecule N2o4 has a greater entropy than NO2

[a.a]

Homework Statement

Why is this statement false?

'Two moles of a substance at temperature T and pressure p has twice the entropy of one mole of the same substance at the same temperature and pressure.'
--> Is it because the number of moles doesn't matter. Why doesn't it?

Why is this statement true?

'The entropy change for the reaction N2O4(g) -> 2 NO2(g) is positive.'
--> The molecule N2o4 has a greater entropy than NO2, so it delta S, change in entropy would be entropy of NO2 - entropy of N2O4, which would be a negative (smaller - bigger number)? Am I going about this wrong?

 

[Mapes]

Why is this statement false?

'Two moles of a substance at temperature T and pressure p has twice the entropy of one mole of the same substance at the same temperature and pressure.'

It's not false; entropy is an extensive variable.

 

[a.a]

If there are more moles in the same place under the same tempreature and pressure, wouldn't that decrease the entropy?

 

[Mapes]

Nope.