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