For the conversion of ice to water at 0°C and 1 atm,

Question

Quizplus · Accepted Answer

During the conversion of ice to water at 0°C and 1 atm, the system absorbs heat from the surroundings, which increases the internal energy of the system (i.e., ΔH is positive). However, the conversion leads to an increase in the entropy of the system because the water molecules in liquid state are more disordered than those in solid ice (i.e., ΔS is positive). As the process occurs at a constant temperature and pressure, we can use the equation ΔG = ΔH - TΔS, where ΔG is the change in Gibbs free energy, T is temperature, and ΔS is the change in entropy. Since ΔH is positive and ΔS is positive, the sign of ΔG will depend on the temperature. At 0°C, the value of T is 273 K, and there is a slight negative value of ΔG indicating that the reaction is spontaneous (i.e., ΔG is zero or negative). Therefore, the correct choice is B.

For the Conversion of Ice to Water at 0°C and 1