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: A sample of an unknown gas effuses in 11.1 min. An equal volume of H 2 in the same apparatus under the same conditions effuses in 2.42 min. What is the molar mass of the unknown gas?

Solution: A sample of an unknown gas effuses in 11.1 min. An equal volume of H 2 in the same apparatus under the same conditions effuses in 2.42 min. What is the molar mass of the unknown gas?

Problem

A sample of an unknown gas effuses in 11.1 min. An equal volume of H 2 in the same apparatus under the same conditions effuses in 2.42 min. What is the molar mass of the unknown gas?

Solution

Concept: Graham's Law of Effusion

Use the graham's law of effusion equation to find molar mass of unknown gas.

First will have to find the rate of effusion of each, since only times are given.

We will assume that we have 1 L of each gas, however you can pick any value for volume, as long as the two volumes are the same for both gases.

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