Difference between revisions of "Molar heat capacity"

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In adiabatic compression (<math>\Delta Q=0</math>) of an ideal gas, <math>PV^\gamma</math> stays constant, where <math>\gamma=\frac{c_V+R}{c_V}</math>.
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In adiabatic compression (<math>\Delta Q=0</math>) of an ideal gas, <math>PV^\gamma</math> stays constant, where <math>\gamma=\frac{c_V+R}{c_V}</math>. An excellent derivation of this can be found [https://www.animations.physics.unsw.edu.au/jw/Adiabatic-expansion-compression.htm here].

Revision as of 04:35, 27 November 2019

Adding heat to a substance changes its temperature in accordance to \[\Delta Q=nc_M\Delta T\] $\Delta Q=$ change in heat
$n=$ moles of substance
$c_M=$ molar heat capacity
$\Delta T=$ change in temperature

At constant volume, $c_M=c_V$.
At constant pressure, $c_M=c_P$.

For an ideal gas, $c_P=c_V+R$ where $R=$ the ideal gas constant.
For an incompressible substance, $c_P=c_V$.

In adiabatic compression ($\Delta Q=0$) of an ideal gas, $PV^\gamma$ stays constant, where $\gamma=\frac{c_V+R}{c_V}$. An excellent derivation of this can be found here.

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