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: The following reaction has KP = 4.50 × 10−5 at 720 K. N2(g) + 3H2(g) ⇌ 2NH3(g) If a reaction vessel is filled with each gas to the partial pressures listed, in which direction will it shift to reach e

Solution: The following reaction has KP = 4.50 × 10−5 at 720 K. N2(g) + 3H2(g) ⇌ 2NH3(g) If a reaction vessel is filled with each gas to the partial pressures listed, in which direction will it shift to reach e

Problem

The following reaction has KP = 4.50 × 10−5 at 720 K. 

N2(g) + 3H2(g) ⇌ 2NH3(g) 

If a reaction vessel is filled with each gas to the partial pressures listed, in which direction will it shift to reach equilibrium? P(NH3) = 93 atm, P(N2) = 48 atm, and P(H2) = 52

Solution

Chemical equilibrium is a form of dynamic equilibrium. This means that although the equilibrium concentrations of reaction components appear static, the reaction is not static. This is because of the fact that at equilibrium individual rates of forward and reverse reactions are equal and the amount of reactants that depletes to yield products is recuperated by the conversion of products back into reactants through a reverse reaction.


This equilibrium can be disturbed through the application of stress on the system, such as the increase in the concentration of either of reactants or the products or changes in temperature.


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