Consider the melting of one mole of water. Use the following data to answer the

Consider
the melting of one mole of water. Use the following data to answer the
questions:S?=(
H2O l)=69.9J/K.mol S?( H2O
s)=47.8J/K.mol ?H?( H2O l)=-285.8kJ/mol and ?H?( H2O
s)=-298.8kJ/mol. Assume standard molar entropies and enthalpies of formation are not functions of temperature in this
range. a) calculate the entropy change of the system for melting ice at -5?C.
b) Calculate the entropy change of the surrounding for melting ice at -5?Cand C) Is this reaction spontaneous at -5?C?
Justify.
next:

The
heat capacity is critical in calculating the enthalpy and entropy. Using the
data (heat capacity) from book or internet and also?fusH (I2)
= 15.52387kJ/mol at 387K and?vap
(I2) =41.57kJ/mol at 457K.a) Calculate the heat required to bring one
mole of iodine from 0K to 500k. b) calculate the absolute entropyof iodine at 500K