Ch. 17 - Chemical ThermodynamicsWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Calculate ΔG° for the reaction NH4NO3(s) → NH4+(aq) + NO3−(aq) to determine whether the reaction is spontaneous or not. Temperature: 298.15 K and ΔS°: 108.7 J/K•molCompound          ΔHf° (kJ/mol)NH4NO3(s)          −365.56NH4+(aq)             −132.51NO3−(aq)             −205.0A.  4.4 J , nonspontaneousB.  – 4.4 kJ, spontaneousC.  28.5 kJ spontaneousD.  −28.5 J nonspontaneousE.  5.6 kJ nonspontaneous 

Problem

Calculate ΔG° for the reaction NH4NO3(s) → NH4+(aq) + NO3(aq) to determine whether the reaction is spontaneous or not. Temperature: 298.15 K and ΔS°: 108.7 J/K•mol

Compound          ΔHf° (kJ/mol)

NH4NO3(s)          −365.56

NH4+(aq)             −132.51

NO3(aq)             −205.0

A.  4.4 J , nonspontaneous

B.  – 4.4 kJ, spontaneous

C.  28.5 kJ spontaneous

D.  −28.5 J nonspontaneous

E.  5.6 kJ nonspontaneous