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: 2S(s) + 3O 2(g) → 2SO3(g) + heatThe rate of this reaction could be increased byA. Decreasing temperatureB. Adding a catalystC. Increasing the concentration of S(s)D. Increasing the concentration of SO 3(g)

Solution: Consider the following reaction: 2S(s) + 3O 2(g) → 2SO3(g) + heatThe rate of this reaction could be increased byA. Decreasing temperatureB. Adding a catalystC. Increasing the concentration of S(s)D. I

Problem

Consider the following reaction: 2S(s) + 3O 2(g) → 2SO3(g) + heat

The rate of this reaction could be increased by

A. Decreasing temperature

B. Adding a catalyst

C. Increasing the concentration of S(s)

D. Increasing the concentration of SO 3(g)

Solution

We’re asked to determine which conditions would increase the rate of this reaction between sulfur and oxygen gas.

Additionally, remember the Le Chatelier’s principle: If a system (chemical reaction) is at equilibrium and we disturb it then the system will readjust to maintain it’s equilibrium state.

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