When 44.0 g of solid carbon dioxide at 1.00 atm pressure are reversibly converted to vapour at
1 atm pressure and −78 °C, 25.33 kJ of heat are absorbed by the system. The density of solid
CO2 is 1.56 g cm−3.

What is the change in G and if S° of CO2(g) is 197.7 J K−1 mol−1 at −78 °C, what is the standard entropy of solid CO2?

Question

When 44.0 g of solid carbon dioxide at 1.00 atm pressure are reversibly converted to vapour at
1 atm pressure and −78 °C, 25.33 kJ of heat are absorbed by the system. The density of solid
CO2 is 1.56 g cm−3. 

What is the change in G and if S° of CO2(g) is 197.7 J K−1 mol−1 at −78 °C, what is the standard entropy of solid CO2?

anitaasks · Answer

I found that deltaG is 0 and the standard entropy of solid CO2 is 67.70. Does anyone know if this is correct?