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: Consider the arrangement of bulbs shown in the drawing. Each of the bulbs contains a gas at the pressure shown.What is the pressure of the system when all the stopcocks are opened, assuming that the t

Solution: Consider the arrangement of bulbs shown in the drawing. Each of the bulbs contains a gas at the pressure shown.What is the pressure of the system when all the stopcocks are opened, assuming that the t

Problem

Consider the arrangement of bulbs shown in the drawing. Each of the bulbs contains a gas at the pressure shown.

What is the pressure of the system when all the stopcocks are opened, assuming that the temperature remains constant? (We can neglect the volume of the capillary tubing connecting the bulbs.)


Three gas flasks are connected via stopcocks to the same horizontal tube. N2 (1.0 liter, 265 torr) is on the left, Ne (1.0 liter, 800 torr) is in the middle, and H2 (0.5 liters, 532 torr) is on the right.

Solution

We are asked to determine the pressure of the system when all the stopcocks are opened, assuming that the temperature remains constant.

Three gas flasks are connected via stopcocks to the same horizontal tube. N2 (1.0 liter, 265 torr) is on the left, Ne (1.0 liter, 800 torr) is in the middle, and H2 (0.5 liters, 532 torr) is on the right.


According to Boyle’s Law, an inverse relationship exists between pressure and volume assuming the number of molecules (n) and the temperature (T) are both constant.


The relationship for Boyle’s Law can be expressed as follows:

P1V1 = P2V2

where:

P1 and V1 are the initial pressure and volume values

P2 and V2 are the values of the pressure and volume of the gas after the change.

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