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e) What is the value for AG at 283K in cal/mol? f) Is melting ice spontaneous at 283K? g) What about the reverse reaction? Would liquid water spontaneously freeze at 283K? h) Convert 283K to °C .Would you expect ice to melt at this temperature?

e) What is the value for AG at 283K in cal/mol? f) Is melting ice spontaneous at 283K? g) What about the reverse reaction? Would liquid water spontaneously freeze at 283K? h) Convert 283K to °C .Would you expect ice to melt at this temperature?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section16.6: Gibbs Free Energy
Problem 16.10CE
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Hi, 

I only need help with question 3 from e-h

Enthalpy, Entropy, and Free Energy 1. Predict the sign (+/-) for AS for the following processes: a) H20(1) --> H20(s) b) CaCO3(s) --> CaO(s) + CO2(g) c) 2NH3(g) --> 2N2{g) + 3H2(g) d) CHCI3(1) --> CHCI3{g) e) CO(g) + 2H2(g)--> CH3OH(I) 2. Consider the following process: NaCI(s)--> Na"(aq) + Cl(ag) AH = + 4.2 kJ/mol a) Does entropy increase or decrease in this process? b) Under what conditions (temperature) would you expect this process to be spontaneous? 3. The process of melting solid ice to produce water has the following thermodynamic values: AH = +1.44 kcal/mol and AS = +5.26 cal/mol · K . a) What is the value for AG at 263K in cal/mol? b) Is melting ice spontaneous at 263K? c) What about the reverse reaction? Would liquid water spontaneously freeze at 263K? d) Convert 263K to °C .Would you expect ice to melt at this temperature? e) What is the value for AG at 283K in cal/mol? f) Is melting ice spontaneous at 283K? g) What about the reverse reaction? Would liquid water spontaneously freeze at 283K? h) Convert 283K to °C .Would you expect ice to melt at this temperature? i) What is the value for AG at 273K in cal/mol? (Be careful to only use 3 Sig Figs in your calculations) j) Convert 273K to °C . Would you expect ice to melt at this temperature? k) A AG of 0 indicates a system is at equilibrium. Use this to explain which process is spontaneous at 273K, melting or freezing? 4. Consider the following process: 2Hg(0) + O2(g)--> 2H9O(s) AH = - 43 kcal/mol a) Does entropy increase or decrease in this process? b) Under what conditions (temperature) would you expect this process to be spontaneous?
Transcribed Image Text:Enthalpy, Entropy, and Free Energy 1. Predict the sign (+/-) for AS for the following processes: a) H20(1) --> H20(s) b) CaCO3(s) --> CaO(s) + CO2(g) c) 2NH3(g) --> 2N2{g) + 3H2(g) d) CHCI3(1) --> CHCI3{g) e) CO(g) + 2H2(g)--> CH3OH(I) 2. Consider the following process: NaCI(s)--> Na"(aq) + Cl(ag) AH = + 4.2 kJ/mol a) Does entropy increase or decrease in this process? b) Under what conditions (temperature) would you expect this process to be spontaneous? 3. The process of melting solid ice to produce water has the following thermodynamic values: AH = +1.44 kcal/mol and AS = +5.26 cal/mol · K . a) What is the value for AG at 263K in cal/mol? b) Is melting ice spontaneous at 263K? c) What about the reverse reaction? Would liquid water spontaneously freeze at 263K? d) Convert 263K to °C .Would you expect ice to melt at this temperature? e) What is the value for AG at 283K in cal/mol? f) Is melting ice spontaneous at 283K? g) What about the reverse reaction? Would liquid water spontaneously freeze at 283K? h) Convert 283K to °C .Would you expect ice to melt at this temperature? i) What is the value for AG at 273K in cal/mol? (Be careful to only use 3 Sig Figs in your calculations) j) Convert 273K to °C . Would you expect ice to melt at this temperature? k) A AG of 0 indicates a system is at equilibrium. Use this to explain which process is spontaneous at 273K, melting or freezing? 4. Consider the following process: 2Hg(0) + O2(g)--> 2H9O(s) AH = - 43 kcal/mol a) Does entropy increase or decrease in this process? b) Under what conditions (temperature) would you expect this process to be spontaneous?
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