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 oxidation of sulfur dioxide by oxygen to sulfur trioxide has been implicated as an important step in the formation of acid rain:2 SO2(g) + O2(g) ⇌ 2 SO3(g)If the equilibrium partial pressures of SO2, O2 and SO3 are 0.564 atm, 0.102 atm and 0.333 atm, respectively at 1000 K, what is Kp at this temperature?A. 0.292 B. 3.42 C. 5.79 D. 8.11E. 6.05

Problem

The oxidation of sulfur dioxide by oxygen to sulfur trioxide has been implicated as an important step in the formation of acid rain:

2 SO2(g) + O2(g) ⇌ 2 SO3(g)

If the equilibrium partial pressures of SO2, O2 and SO3 are 0.564 atm, 0.102 atm and 0.333 atm, respectively at 1000 K, what is Kp at this temperature?

A. 0.292 

B. 3.42 

C. 5.79 

D. 8.11

E. 6.05

Solution

We’re being asked to determine the equilibrium constant (Kp) at 1000 K for this reaction:


2 SO2(g) + O2(g) ⇌ 2 SO3(g)


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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