Question

Calculate the entropy change in melting 1 mole of ice at 273 K, \( \Delta H_f^o = 6.025 \, \text{kJ/mol} \):

• A. 11.2 J K\(^{-1}\) mol\(^{-1}\)
• B. 22.1 J K\(^{-1}\) mol\(^{-1}\)
• C. 15.1 J K\(^{-1}\) mol\(^{-1}\)
• D. 5.1 J K\(^{-1}\) mol\(^{-1}\)

Hint:

The entropy change during a phase transition is given by the ratio of heat involved and the temperature at which the phase change occurs.

Answer 1

The Correct Option is A

The entropy change \( \Delta S \) is calculated using the formula: \[ \Delta S = \frac{\Delta H_f^o}{T} \] Substituting the values \( \Delta H_f^o = 6.025 \, \text{kJ/mol} \) and \( T = 273 \, \text{K} \), we get \( \Delta S = 11.2 \, \text{J/mol·K} \).
Final Answer: \[ \boxed{11.2 \, \text{J/mol·K}} \]