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: Oxygen can be produced in the laboratory by the reaction 2KClO3(s) → 2KCl(s) + 3O2(g) .How much potassium chlorate is needed to produce 2.75 L of oxygen, collected over water at 37°C and 94.9 kPa? The vapor pressure of water at 37°C is 6.28 kPa.1. 0.189 mol2. 9.45 × 10−2 mol3. 0.142 mol4. 7.20 × 10−2 mol5. 6.30 × 10−2 mol

Problem

Oxygen can be produced in the laboratory by the reaction 

2KClO3(s) → 2KCl(s) + 3O2(g) .

How much potassium chlorate is needed to produce 2.75 L of oxygen, collected over water at 37°C and 94.9 kPa? The vapor pressure of water at 37°C is 6.28 kPa.

1. 0.189 mol

2. 9.45 × 10−2 mol

3. 0.142 mol

4. 7.20 × 10−2 mol

5. 6.30 × 10−2 mol