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Magazine Chapter 6: Problem 6
If a system is not adiabatic, then heat leaves or enters the system. What is the immediate response of a system (a) in liquid-gas equilibrium if heat is removed? (b) in solid-gas equilibrium if heat is added? (c) in liquid-solid equilibrium if heat is removed? (d) composed entirely of solid phase if heat is removed?
Short Answer
Expert verified
(a) Gas condenses into liquid. (b) Solid sublimes to gas. (c) Liquid freezes to solid. (d) Solid cools down.
Step by step solution
01
Understand Liquid-Gas Equilibrium
In a liquid-gas equilibrium, both phases exist together. If heat is removed, energy is extracted from the system.
02
Effect on Liquid-Gas Equilibrium
Removing heat in liquid-gas equilibrium causes the gas to condense into liquid, as the system loses energy needed to maintain the gaseous phase.
03
Understand Solid-Gas Equilibrium
In solid-gas equilibrium, the solid phase is in equilibrium with its gaseous form. Adding heat increases the energy of the system.
04
Effect on Solid-Gas Equilibrium
If heat is added, the solid sublimes or converts into the gaseous phase due to increased energy, pushing more solid to change into gas.
05
Understand Liquid-Solid Equilibrium
In a liquid-solid equilibrium, the liquid and solid phases coexist. Removing heat affects this balance.
06
Effect on Liquid-Solid Equilibrium
Removing heat from a liquid-solid equilibrium system causes the liquid to freeze into the solid state, as the system energy decreases.
07
Analyze Solid Phase System
For a system entirely in the solid phase, removing heat affects the internal energy of the solid.
08
Effect on Solid Phase
Removing heat from a solid leads to a decrease in its internal energy, causing it usually to just cool or potentially enter a different crystal lattice form at low temperatures, depending on material properties.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Liquid-Gas Equilibrium
In a liquid-gas equilibrium, both the liquid and gas phases exist together in balance. This balance is maintained by the continuous evaporation and condensation processes. When heat is removed from such a system, energy is simultaneously withdrawn. This results in a tendency for the gaseous molecules to lose energy and condense back into the liquid phase. This process continues until a new equilibrium state is achieved at a lower temperature. The reduced energy in the system means fewer molecules have the necessary energy to remain in the gaseous phase. Hence, in liquid-gas equilibrium, removing heat leads to condensation.
Solid-Gas Equilibrium
In the solid-gas equilibrium, the solid and its gaseous form coexist. This can often be seen in processes like sublimation, where a solid transitions directly into a gas without passing through the liquid phase. When heat is added to a solid-gas equilibrium system, the energy within the system increases. This additional energy allows more solid molecules to achieve the energy levels necessary to transition into the gaseous phase. As a result, the solid begins to sublime more rapidly, enhancing the amount of gas-phase substance in the equilibrium mix. Thus, adding heat results in increased sublimation.
Liquid-Solid Equilibrium
Liquid-solid equilibrium involves a balance where both liquid and solid phases coexist, such as in melting ice. Removing heat from this system extracts energy, disrupting the balance. As a result, the liquid molecules lose energy, leading to freezing and creation of more solid. The shift from liquid to solid continues as long as heat is being removed. Eventually, the system reaches a new equilibrium at a lower temperature, with more mass present in the solid phase compared to the liquid phase. Therefore, in liquid-solid equilibrium, removing heat primarily causes freezing.
Heat Transfer
Heat transfer is a fundamental concept in understanding phase equilibrium processes. It involves the movement of thermal energy from one object or substance to another. There are three primary modes of heat transfer: conduction, where energy moves through a solid; convection, where energy is transferred through fluids; and radiation, where energy is transferred through electromagnetic waves. In the context of phase equilibrium, heat transfer dictates how quickly and effectively phases change, such as solid to liquid or liquid to gas, impacting the equilibrium point. Heat transfer plays a crucial role in energy distribution across phases.
Thermodynamics
Thermodynamics is the science of energy and its transformations. It provides the theoretical framework for understanding how energy transfers impact matter in various phases. In phase equilibrium, thermodynamics helps predict how a system reacts when subjected to changes in temperature or pressure. The laws of thermodynamics govern these changes:
- The First Law, which states that energy cannot be created or destroyed, only transformed.
- The Second Law, which introduces the concept of entropy, suggesting that systems naturally progress towards disorder.
- The Third Law, which implies that as temperature approaches absolute zero, the entropy of a perfect crystal approaches zero.
