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: Samples containing equal numbers of moles of H 2, N2, O2, and He are placed into separate 1 L containers at the same temperature. Assuming each gas behaves ideally, which container has the highest pre

Solution: Samples containing equal numbers of moles of H 2, N2, O2, and He are placed into separate 1 L containers at the same temperature. Assuming each gas behaves ideally, which container has the highest pre

Problem

Samples containing equal numbers of moles of H 2, N2, O2, and He are placed into separate 1 L containers at the same temperature. Assuming each gas behaves ideally, which container has the highest pressure?

a. H2

b. N2

c. O2

d. He

e. All the gases would all exhibit the same pressure.

Solution

We’re given equal moles of H2, N2, O2, and He in separate 1-L containers at the same temperature. We’re being asked which container has the highest pressure, assuming each gas behaves ideally.


Recall that the ideal gas law is:



View the complete written solution...