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: In the Haber process, N2 (g) + 3H2 (g) → 2NH3 (g)ΔG° at 298 K for this reaction is -33,300 J/mol.The value of ΔG at 298 K for a non-equilibrium reaction mixture that consists of 1.9 atm N  2, 1.6 atm H2, and 0.65 atm NH 3 is __________.a. -40,500 Jb. -1,800 Jc. -7.25 × 106 Jd. -3.86 × 106 Je. -104,500 J 

Problem

In the Haber process, N2 (g) + 3H2 (g) → 2NH3 (g)
ΔG° at 298 K for this reaction is -33,300 J/mol.

The value of ΔG at 298 K for a non-equilibrium reaction mixture that consists of 1.9 atm N  2, 1.6 atm H2, and 0.65 atm NH 3 is __________.

a. -40,500 J
b. -1,800 J
c. -7.25 × 106 J
d. -3.86 × 106 J
e. -104,500 J