Question

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged you don't have enough information to decide, check the not en-ugh information" button in the last column. A few grams of water vapor (Ho) The water condenses to a liquid at a constant temperature of 3.0C not enough The helun is heated from 7.ONC to Δ5·0 A few moles of helium (He) gas. volume of 1.O L to a volume of not enough The carbon diaxide is heated from ○ △S > 0 3 MacBook Air 名D

Answer 1

Case 1

You must consider here that a gaseous substance has more energy than a liquid one, and also more entropy. In this case, the initial entropy is bigger than the final one, therefore dS <0

Case 2

In this case you have an increment in the energy of the substance, as well as an expansion, in which the molecules are more dispersed too. The initial entropy is lower than the final, therefore dS>0

Case 3

Considering that the dS in this scenario is dependent on Temperature and Volume, even when the volume is a constant, the temperature is increasing and therefore more energy is being held in the constant volume container. In this case, it is very likely that the initial entropy is lower than the final one, therefore dS>0