At 10 C ice changes to water. H 2 O(s) H 2 O(l) H =

At 10 °C ice changes to water.

H₂O(s) → H₂O(l)                                                         ΔH^θ= +6.01 kJ mol^–1

a. Explain why the entropy change of the system is positive.

b. The entropy change for the system is +22.0 J K^–1 mol^–1. Calculate the total entropy change at 10.0 °C.

c. Explain why the process shown in the equation does not occur at –10.0 °C.

d. At 273K ice and water are in equilibrium. 

H₂O(s) ⇌ H₂O(l)                                                     ΔH^θ= +6.01 kJ mol–1

i. Calculate the entropy change of the surroundings for this process.

ii. What main assumption did you make when doing this calculation?

iii. Use your answer to part d i to deduce the value of ΔS_system at 278 K. Explain your answer fully.

e. At –10.0 °C, the value of ΔS_system is –22.0 J K^–1 mol^–1 and the value of ΔS_surroundings is +22.9 J K^–1 mol^–1. Calculate the total entropy change in the process. Include the correct sign.