The heat capacity is critical in calculating the enthalpy and entropy. Using the data (heat capacity) from book or internet and also ?fus H (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 entropy of iodine at 500K
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.
The heat capacity is critical in calculating the enthalpy and entropy. Using the data (heat capacity) from book or internet and also ?fus H (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 entropy of iodine at 500K
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?C and C) Is this reaction spontaneous at -5?C? Justify.
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