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: An atmospheric chemist studying the pollutant SO2 places a mixture of SO2 and O2 in a 2.00-L container at 800. K and 1.90 atm. When the reaction occurs, gaseous SO3 forms, and the pressure falls to 1.

Solution: An atmospheric chemist studying the pollutant SO2 places a mixture of SO2 and O2 in a 2.00-L container at 800. K and 1.90 atm. When the reaction occurs, gaseous SO3 forms, and the pressure falls to 1.

Problem

An atmospheric chemist studying the pollutant SO2 places a mixture of SO2 and O2 in a 2.00-L container at 800. K and 1.90 atm. When the reaction occurs, gaseous SO3 forms, and the pressure falls to 1.65 atm. How many moles of SO3 form?

Solution

SO2 and O2 react to form SO3:

SO2(g) + O2(g) → SO3(g)

Balancing this gives us:

2 SO2(g) + O2(g) → 2 SO3(g)

Based on the chemical reaction, 3 moles of reactants form 2 moles of product and the total moles of gas decreases by 1 mole.

We can use the ideal gas law to determine the moles of gas before and after the reaction.

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