Question

When ice melts at its normal melting point; 273.16 K and 1 atmosphere; which of the following is true for the process shown?

A) AH < 0, AS > 0, AV >0
8) AH < 0, 4s 0,Av > 0
C) AH > 0, As < 0, AV < 0
D) AH > 0, 4S > 0,Av > 0
E) AH > 0, 4s > 0, AV < 0

Answer 1

During the melting of ice at 0°C and 1 atmosphere, there is a positive change in enthalpy, entropy, and volume (ΔH > 0, ΔS > 0, and ΔV > 0).

Step-by-step explanation:

When ice melts at its normal melting point, which is 273.16 K (0°C) under 1 atmosphere of pressure, the thermodynamic properties associated with this process include a change in enthalpy (ΔH), entropy (ΔS), and volume (ΔV). Considering that melting is an endothermic process, heat is absorbed from the surroundings to break the intermolecular forces in ice, thus ΔH is positive. The change in entropy, ΔS, is also positive because the molecules in the liquid state (water) have more disorder and accessible energy states than in the solid state (ice). The volume increases upon melting, thus ΔV is positive as water is less dense than ice. Therefore, we can conclude that the correct answer is: D) ΔH > 0, ΔS > 0, ΔV > 0.