Question

Use the second law of thermodynamics to explain briefly what happens, in terms of the entropy of the stable phase, when the temperature of ice is raised from -10 °C to 10 °C.

Answer 1

As the temerature of ice changes from -10⁰ c to 10⁰c, the ice changes spontaneously to water by the following equation,

H2O (s) + Heat ---------> H2O (l),

the ice absorbed some amount of heat and it becomes liquid , means there is decrease in entropy of the system,

the second law of thermodynamic states that the process in which transfer of matter and energy between bodies of matter, here heat is absorbed by the system. the ice has more ordered structure and increase in entropy , but at liquid water the entropy of system decreases.,

it can be explained by the latent heat of fusion = Q=mL,

Q= HEAT ABSORBED BY THE ICE, L= LATENT HEAT OF FUSION, m= mass of ice,

Delta S=Q/T=mL/T,

Where T= temp. in K,

that Delta S is less at above 0⁰C and more at below 0⁰c,

as going from -10 to 10⁰c, entropy will le less.