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  5. Chemistry (CHPV200)

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THERMODYNAMICS: ADIABATIC PROCESSES
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The notes are for the thermodynamics in chemistry. They explain the adiabatic processes in detail and also they consists of worked examples and self test exercises

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  • November 13, 2022
  • 8
  • 2022/2023
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UNIT 5 ADIABATIC PROCESSES
AIM: To determine thermodynamic quantities (ΔU, ΔH, q, w and ΔT) for adiabatic
processes


The two kinds of processes frequently encountered in the laboratory and in
thermodynamic arguments
Isothermal processes:




Temp
control
unit



dT = 0
reaction


water bath




Adiabatic processes
Heat cannot enter or leave the system, such that dq = 0




A typical Dewar container
McGraw-Hill Concise Encyclopedia of Engineering. © 2002 by The McGraw-Hill Companies, Inc.

, The pressure-volume relationship for ideal, reversible adiabatic expansion of a
gas


Pext2

counterweight
Pext1 P2


P1



Thermally insulated wall


P1, V1, T1 → P2, V2, T2

Heat cannot flow into or out of system: dq =0
From first law of thermodynamics : dU = dq + dw
dU = dw (1)
For reversible expansion of n moles of ideal gas, the infinitesimal change in internal
energy (dU) wil cause infinitesimal change in temperature (dT):


𝑑𝑈 = 𝑛𝐶𝑣 𝑑𝑇
(2)
The infinitesimal work done (dw) will cause infinitesimal volume change (dV)

𝑑𝑤 = −𝑃𝑑𝑉
The expansion is for an ideal gas under reversible condition. The ideal gas equation
is therefore incorporated:
1
𝑑𝑤 = −𝑛𝑅𝑇 ( ) 𝑑𝑉
𝑉
(3)
From equa 1 condition, equations 2 and 3 can be set equal:
1
𝑛𝐶𝑣 𝑑𝑇 = −𝑛𝑅𝑇 ( ) 𝑑𝑉
𝑉

(4)

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