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Two different kinds of heat capacity exist; heat capacity at constant pressure and heat capacity at constant volume. Researchers have reported that, for gases; Cp > Cv. As an example, for ideal gases,Cp - Cv =R where R is the universal gas constant. The heat capacity at constant pressure for ideal gasses is approximately 30-60 % larger than the heat capacity at constant volume. Using undergraduate thermodynamics argument, explain why Cp is larger than Cv  for gases. Note:   Cp = (dQ/dT)p  and Cv = (dQ/dT)v

Two different kinds of heat capacity exist; heat capacity at constant pressure and heat capacity at constant volume. Researchers have reported that, for gases; Cp > Cv. As an example, for ideal gases,Cp - Cv =R where R is the universal gas constant. The heat capacity at constant pressure for ideal gasses is approximately 30-60 % larger than the heat capacity at constant volume. Using undergraduate thermodynamics argument, explain why Cp is larger than Cv  for gases. Note:   Cp = (dQ/dT)p  and Cv = (dQ/dT)v

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
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Two different kinds of heat capacity exist; heat capacity at constant pressure and heat capacity at constant volume. Researchers have reported that, for gases; Cp > Cv. As an example, for ideal gases,Cp - Cv =R where R is the universal gas constant. The heat capacity at constant pressure for ideal gasses is approximately 30-60 % larger than the heat capacity at constant volume. Using undergraduate thermodynamics argument, explain why Cp is larger than Cv  for gases.

Note:  

Cp = (dQ/dT)p  and Cv = (dQ/dT)v

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