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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: When KClO3(s) (molar mass = 122.55 g mol–1 ) is heated at high temperature, it decomposes to give KCl(aq) (molar mass = 74.55 g mol–1 ) and O2(g) (molar mass = 32.00 g mol–1 ) as products. If 4.289 g of KClO3 are heated, how many liters of oxygen gas (measured at 22.4 oC and 754.0 torr) are produced?A. 1.283 L B. 0.9626 L C. 0.8555 L D. 1.668 L E. 1.925 L

Problem

When KClO3(s) (molar mass = 122.55 g mol–1 ) is heated at high temperature, it decomposes to give KCl(aq) (molar mass = 74.55 g mol–1 ) and O2(g) (molar mass = 32.00 g mol–1 ) as products. If 4.289 g of KClO3 are heated, how many liters of oxygen gas (measured at 22.4 oC and 754.0 torr) are produced?

A. 1.283 L 

B. 0.9626 L 

C. 0.8555 L 

D. 1.668 L 

E. 1.925 L

Solution

Write the balanced equation and determine the moles of Oproduced from 4.289 g KClO3 using gas stoichiometry. Lastly, use ideal gas equation to determine the volume of O2 from the # of moles O2 produced

The initial and unbalanced equation of decomposition of KClO3 will appear as:

KClO3 → O2 + KCl

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