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, Kp for the reaction,Br2(g) <=> 2 Br(g) is 3,498.Calculate the value of Kp for the reaction,1/2 Br2(g) ) <=> Br(g)


At a certain temperature, Kp for the reaction,

Br2(g) <=> 2 Br(g) is 3,498.

Calculate the value of Kp for the reaction,

1/2 Br2(g) ) <=> Br(g)


We’re being asked to determine the equilibrium constant at 458 ˚C for this reaction:

1/2 Br2(g) Br(g)

Given another reaction with it's Kp

Br2(g) 2 Br(g) is 3,498

Recall that the equilibrium constant is the ratio of the products and reactants

We use Kp when dealing with pressure and Kc when dealing with concentration:

Kp=PproductsPreactants     Kc=[products][reactants]

Note that solid and liquid compounds are ignored in the equilibrium expression.

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