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: Use the molar volume of a gas at STP to calculate the density (in g/L) of oxygen gas at STP.

Solution: Use the molar volume of a gas at STP to calculate the density (in g/L) of oxygen gas at STP.

Problem

Use the molar volume of a gas at STP to calculate the density (in g/L) of oxygen gas at STP.

Solution

We’re being asked to calculate the density (in g/L) of O2 gas at standard temperature and pressure.


Recall that density is the ratio of the mass and volume of an object:


density=massvolume



Also, recall that standard temperature and pressure (STP) is defined as 1 atm and 0 ˚C

We can use the ideal gas law to determine the volume occupied by 1 mole of any gas at STP:


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