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: At a certain temperature, the equilibrium constant K c for this reaction is 53.3.H2 + I 2 → 2 HIAt this temperature, 0.800 mol of H2 and 0.800 mol of I2 were placed in 1.00L container to react. What c

Solution: At a certain temperature, the equilibrium constant K c for this reaction is 53.3.H2 + I 2 → 2 HIAt this temperature, 0.800 mol of H2 and 0.800 mol of I2 were placed in 1.00L container to react. What c

Problem

At a certain temperature, the equilibrium constant K c for this reaction is 53.3.

H2 + I 2 → 2 HI

At this temperature, 0.800 mol of H2 and 0.800 mol of I2 were placed in 1.00L container to react. What concentration of HI is present at equilibrium?

Solution

We’re given the following equilibrium reaction:

H2 + I2(g)  2 HI; Kc = 53.3


We know that the initial amount of H2 and I2 is 0.800 mol. In a 1.00 L container, the concentration of each is:



From this, we can construct an ICE table:



The Kc expression for the reaction is:



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