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 4.0 moles of helium gas is confined to a 24.0 Liter balloon at 176 °C at 6.0 atm. The balloon expands while temperature remains constant to 36.0 Liters. What is the new pressure?A) 2.0 atmB) 3.0 atmC) 4.0 atmD) 8.0 atmE) 9.0 atm

Problem

A sample of 4.0 moles of helium gas is confined to a 24.0 Liter balloon at 176 °C at 6.0 atm. The balloon expands while temperature remains constant to 36.0 Liters. What is the new pressure?

A) 2.0 atm

B) 3.0 atm

C) 4.0 atm

D) 8.0 atm

E) 9.0 atm

Solution

We are asked to calculate the new pressure when a 24.0 L at 6.0 atm expands to 36.0 L at a constant temperature. 

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


Solution BlurView Complete Written Solution