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: If the pressure in a helium-filled balloon is 4.4 atm when filled to 5.0 × 10  2 L, what volume is occupied by the helium-filled balloon when the pressure is reduced to 1.1 atm?(a) 2.0 × 102 L(b) 2.5 × 102 L(c) 2.2 × 102 L(d) 2.0 × 103 L(e) 3.0 × 102 L

Problem

If the pressure in a helium-filled balloon is 4.4 atm when filled to 5.0 × 10  2 L, what volume is occupied by the helium-filled balloon when the pressure is reduced to 1.1 atm?

(a) 2.0 × 102 L

(b) 2.5 × 102 L

(c) 2.2 × 102 L

(d) 2.0 × 103 L

(e) 3.0 × 102 L

Solution

Helium inside a balloon was initially at 4.4 atm when filled to 5.0 × 10  2 L then the pressure was reduced to  1.1 atm at a constant temperature. We’re being asked to determine the volume of the gas after decreasing the pressure.


Recall that the ideal gas law is:


PV=nRT


The pressure and volume of a gas are related to the number of moles, gas constant and temperatureThe value nRT is constant


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