Ch. 17 - Chemical ThermodynamicsWorksheetSee all chapters
All Chapters
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: For which reaction, carried out at standard conditions, would both the enthalpy and entropy changes drive the reaction in the same direction? a) 2 H2 (g) + O2 (g) → 2 H2O (l)         ΔH = - 571.1 kJ b) 2 Na (s) + Cl2 (g) → 2 NaCl (s)      ΔH = - 822.0 kJ c) N2 (g) + 2 O2 (g) → 2 NO2 (g)        ΔH = + 67.7 kJ d) 2 NH3 (g) → N2 (g) + 3 H2 (g)        ΔH = + 92.4 kJ

Problem

For which reaction, carried out at standard conditions, would both the enthalpy and entropy changes drive the reaction in the same direction?

a) 2 H(g) + O(g) → 2 H2O (l)         ΔH = - 571.1 kJ

b) 2 Na (s) + Cl(g) → 2 NaCl (s)      ΔH = - 822.0 kJ

c) N(g) + 2 O(g) → 2 NO(g)        ΔH = + 67.7 kJ

d) 2 NH(g) → N(g) + 3 H(g)        ΔH = + 92.4 kJ