Question

what is the change in entropy (δ s) when an icicle melts at 2°c? a. δ s= δ h b. δ s> 0 c. δ s< 0 d. δ s= 0

Explanation:

When an icicle (solid water) melts into liquid water at \(2^\circ\text{C}\), the system goes from a more ordered state (solid) to a less ordered state (liquid). Entropy (\(S\)) is a measure of disorder or randomness. An increase in disorder means an increase in entropy, so \(\Delta S>0\) (since the final entropy of liquid water is greater than the initial entropy of the icicle). Option A is incorrect because \(\Delta S=\frac{\Delta H}{T}\) (at constant temperature) and not \(\Delta S = \Delta H\). Option C is wrong as entropy increases, not decreases. Option D is incorrect because a phase change (melting) involves a change in entropy (it's not a reversible adiabatic process where \(\Delta S = 0\)).

Answer:

B. \(\Delta S>0\)