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 gas sample contains 3.50 moles of argon, 2.08 moles of neon and 1.22 moles of nitrogen. If the total pressure of the sample is 3.66 atm, what is the partial pressure of argon?(A) 3.66 atm (B) 22.4 atm (C) 0.179 atm (D) 1.12 atm (E) 1.88 atm

Problem

A gas sample contains 3.50 moles of argon, 2.08 moles of neon and 1.22 moles of nitrogen. If the total pressure of the sample is 3.66 atm, what is the partial pressure of argon?

(A) 3.66 atm 

(B) 22.4 atm 

(C) 0.179 atm 

(D) 1.12 atm 

(E) 1.88 atm

Solution

We’re being asked to calculate the partial pressure of Ar in a mixture of N2, Ne, and Ar


Recall that the partial pressure of a gas (PGas) in a mixture is given by:


Pgas = χgasPtotal

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