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Calculating the enthalpy and entropy

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.

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

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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 o

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Chemistry: Calculating the enthalpy and entropy

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Solution Preview :

Prepared by a verified Expert

Chemistry: Calculating the enthalpy and entropy

Reference No:- TGS0691367

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