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: Calcium carbonate can be converted to quick lime by the following reaction:CaCO3(s) → CaO(s) + CO2(g) Given that:       for CaCO3(s)  at 25°C     ΔHf° = -1206.9 kJ/mol  ΔS° = 92.9 J/mol K,                        for CaO(s)                     ΔHf° = -635.5 kJ/mol      ΔS° = 39.8 J/mol  K                        for CO2(g))                     ΔHf° = -393.5 kJ/mol     ΔS° = 213.6 J/mol  K Use these data to calculate ΔGo  for the reaction.A)  225.7 kJ/mole         B)   130.1 kJ/mole   C) -130.1 kJ/mole    D)    -225.7 kJ/mole      E)  none of these 

Problem

Calcium carbonate can be converted to quick lime by the following reaction:

CaCO3(s) → CaO(s) + CO2(g)

 

Given that:       for CaCO3(s)  at 25°C     ΔHf° = -1206.9 kJ/mol  ΔS° = 92.9 J/mol K,

                        for CaO(s)                     ΔHf° = -635.5 kJ/mol      ΔS° = 39.8 J/mol  K

                        for CO2(g))                     ΔHf° = -393.5 kJ/mol     ΔS° = 213.6 J/mol  K

 

Use these data to calculate ΔGo  for the reaction.

A)  225.7 kJ/mole         B)   130.1 kJ/mole   C) -130.1 kJ/mole    D)    -225.7 kJ/mole      E)  none of these