Ch. 17 - Chemical ThermodynamicsWorksheetSee all chapters
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: Two different gases occupy two separate bulbs. Consider the process that occurs when the stopcock separating the gases is opened, assuming the gases behave ideally.How does the process affect the enth

Solution: Two different gases occupy two separate bulbs. Consider the process that occurs when the stopcock separating the gases is opened, assuming the gases behave ideally.How does the process affect the enth

Problem

Two different gases occupy two separate bulbs. Consider the process that occurs when the stopcock separating the gases is opened, assuming the gases behave ideally.

How does the process affect the enthalpy of the surroundings?

 Two flasks are shown, connected by a stopcock.  Each contains ten spheres of a single type, but each flask has a different type.

Solution

In this problem, we are asked about how the enthalpy of the surroundings is affected when the two gases are mixed together.

Enthalpy is a thermodynamic property that is defined as:

H=U+PV 

Where is enthalpy, is internal energy, is pressure, and is volume.


And the change in enthalpy (ΔH) is equal to the heat that flows in and out of the system, in which, the enthalpy change of the universe is the sum of the enthalpy change of the system and the surroundings.

𝞓Huniverse=𝞓Hsystem+𝞓Hsurrounding


The system is the region in space that is subject to thermodynamic study. While the surrounding is everything that lies around the system.


To solve this problem, remember that:

ΔHsurr > 0: ΔHsystem < 0, the reaction is exothermic, heat is absorbed by the surrounding, heat is released by the system.

ΔHsurr < 0: ΔHsystem > 0, the reaction is endothermic, heat is absorbed by the system from the surrounding.

ΔHsurr = 0: ΔHsystem = 0, the reaction is neither endothermic nor exothermic, heat is neither lost nor gained.

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