Ch.14 - Chemical EquilibriumWorksheetSee 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: Consider the following reaction at equilibrium:2 NH3 (g) ⇌ N2 (g) + 3 H2 (g)                 ΔH° = + 92.4 kJIncreasing the temperature to the system at equilibrium will ___________________.a) derease the concentration of NH 3 (g) at equilibrium. b) decrease the concentration of H 2 (g) at equilibrium. c) cause no change to the system. d) cause the reaction to shift to the left.e) remove all of the H 2 (g).

Solution: Consider the following reaction at equilibrium:2 NH3 (g) ⇌ N2 (g) + 3 H2 (g)                 ΔH° = + 92.4 kJIncreasing the temperature to the system at equilibrium will ___________________.a) derease

Problem

Consider the following reaction at equilibrium:

2 NH3 (g) ⇌ N2 (g) + 3 H2 (g)                 ΔH° = + 92.4 kJ

Increasing the temperature to the system at equilibrium will ___________________.

a) derease the concentration of NH 3 (g) at equilibrium. 

b) decrease the concentration of H 2 (g) at equilibrium. 

c) cause no change to the system. 

d) cause the reaction to shift to the left.

e) remove all of the H 2 (g).