Question

Which statement is true for the freezing of liquid water below 0 degrees Celsius? a. ΔH is positive; ΔS is negative; ΔG is negative b. ΔH is negative; ΔS is negative; ΔG is negative c. ΔH is positive; ΔS is positive; ΔG is positive d. ΔH is positive; ΔS is negative; ΔG is positive

Answer 1

The correct statement for the freezing of liquid water below 0 degrees Celsius is option d. ΔH is positive; ΔS is negative; ΔG is positive.

Step-by-step explanation:

The correct statement for the freezing of liquid water below 0 degrees Celsius is option d. ΔH is positive; ΔS is negative; ΔG is positive.

When water freezes below 0 degrees Celsius, it undergoes a phase transition from liquid to solid, and this process is endothermic, meaning it requires energy input (ΔH is positive).

Additionally, the freezing of water leads to a decrease in entropy (ΔS is negative) because the solid state has lower randomness and order compared to the liquid state.

The condition ΔG = ΔH - TΔS determines the spontaneity of a process. Since ΔH is positive and ΔS is negative, the term TΔS will be negative at low temperatures, making ΔG positive. Therefore, the process is non-spontaneous (ΔG is positive).