Question A25 Calculate the molar entropy change for the melting of ice, H?O(s), to liquid water, H?O(l) at a temperature of 0 °C and pressure of 1.00 atm. H?O (s) ⇌ H?O (l) The molar enthalpy change for this process is 6.0 kJ mol?¹ A. 3.8 J K?¹ mol?¹ B. -22 J K?¹ mol?¹ C. 22 J K?¹ mol?¹ D. J K?¹ mol?¹ E. 0.32 J K?¹ mol?¹ (3 marks)

Question A25 Calculate the molar entropy change for the melting of ice, H?O(s), to liquid water, H?O(l) at a temperature of 0 °C and pressure of 1.00 atm. H?O (s) $\rightleftharpoons$ H?O (l) The molar enthalpy change for this process is 6.0 kJ mol?¹ A. 3.8 J K?¹ mol?¹ B. -22 J K?¹ mol?¹ C. 22 J K?¹ mol?¹ D. J K?¹ mol?¹ E. 0.32 J K?¹ mol?¹ (3 marks)

Calculate the entropy change for the conversion of following: (a) $1 \mathrm{~g}$ ice to water at $273 \mathrm{~K}, \Delta H_{\mathrm{f}}$ for ice $=6.025 \mathrm{~kJ} \mathrm{~mol}^{-1}$. (b) $36 \mathrm{~g}$ water to vapour at $373 \mathrm{~K} ; \Delta H_{\mathrm{v}}$ for $\mathrm{H}_{2} \mathrm{O}=40.63 \mathrm{~kJ} \mathrm{~mol}^{-1}$.