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

A student adds 0.1727 g of an unknown gas to a 125-mL flask. The pressure of this gas sample is found to be 0.833 atm at 20.0 °C. Is the gas likely to be methane (CH4), nitrogen (N2), oxygen (O2), neon (Ne) or argon (Ar)?

A. CH4 

B. N2 

C. Ne 

D. Ar 

E. O2


Calculate for the number of moles using the ideal gas equation and the given conditions. Divide the calculated moles by the grams provided to determine the molar mass of the gas.

Recall that ideal gas equation:

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