For the of freezing liquid ethanol at a given temperature and pressure,A. ΔH is positive and ΔS is positive.B. ΔH is positive and ΔS is negative.C. ΔH is negative and ΔS is positive.D. ΔH is negative and ΔS is negative.

D. ΔH is negative and ΔS is negative.

Let's break this down:

- ΔH, or change in enthalpy, measures the total heat content of a system and represents the energy used or released during a process. - ΔS, or change in entropy, measures the disorder or randomness in a system.

When liquid ethanol freezes, it goes from a disorderly state (liquid) where the molecules are freely moving around, to a more ordered state (solid) where the molecules are in a fixed lattice structure. Entropy decreases during this process because the solid state is more orderly than the liquid state, which means ΔS is negative.

For the process of freezing, energy is released, as the molecules within ethanol lose energy and form intermolecular bonds. This release of energy signifies that the process is exothermic, meaning ΔH is negative.

So, during the freezing of liquid ethanol, ΔH is negative (energy is released) and ΔS is negative (order increases).