Applications of Thermodynamics

Solids have higher enthalpy than liquids and gases.

Solids are more miscible than liquids and gases.

Solids have equal entropy as liquids and gases.

Solids have lower entropy than liquids and gases.

Shift towards lower probability densities near equilibrium position as partitional contribution from rotational modes becomes relevant

Increased narrowing of positional probabilities due decreased reliance on vibrational states far from equilibrium

No change in positional probabilities since changes in kinetic energy do not affect confinement potentials

Increased broadening of positional probabilities due to higher kinetic energies allowing access to wider range of positions

Ice melting into water at 0°C.

Gas expanding into a vacuum.

A liquid solidifying into solid crystals lattice.

Water Vapor condensing into dew on a grass blade.

Liquid water spontaneously freezing into ice below its freezing point while releasing heat into its surroundings.

Evaporation of ethanol at ambient pressure and temperature resulting from increased vapor pressure above its liquid form.

A hot piece of metal cooling down to room temperature by releasing thermal energy into its environment.

An exothermic reaction where reactants form products that occupy lesser volume than initial substances combined.

There's no change in total entropy since ideal gases don't interact energetically when mixed.

The total entropy increases due to increased molecular randomness upon mixing.

The total entropy decreases as there’s no heat added during mixing.

Total entropy decreases due to decreased pressure after mixing occurs.

Liquid evaporating to gas.

Solid melting into a liquid.

Gas condensing to a liquid.

Ice subliming into vapor.

It decreases

It fluctuates unpredictably

It stays the same

It increases

Remain unchanged as salt simply dissociates

Fluctuates with temperature changes only

It increases due to greater dispersion of ions

Decrease due to interaction between poles decrease

Decreasing the volume of the container.

Introducing a catalyst that speeds up reaction rates.

Adding more gas molecules to the system.

Increasing the pressure by external means.

It fluctuates unpredictably.

It remains constant.

It increases.

It decreases.