Difference between revisions of "Molar heat capacity"

(create article)
 
(restyled/rewrote page source for easier editing/reading and added first sentence and categorized page)
 
(2 intermediate revisions by one other user not shown)
Line 1: Line 1:
Adding heat to a substance changes its temperature in accordance to <cmath>\Delta Q=nc_M\Delta T</cmath>
+
The molar heat capacity is the amount of energy required to change the temperature of an amount of substance by a certain amount per moles of the substance and change in temperature.
<math>\Delta Q=</math> change in heat
 
<math>n=</math> moles of substance
 
<math>c_M=</math> molar heat capacity
 
<math>\Delta T=</math> change in temperature
 
  
At constant volume, <math>c_M=c_V</math>.
+
Adding [[heat]] to a substance changes its temperature in accordance to <cmath>\Delta Q=nc_M\Delta T,</cmath>
At constant pressure, <math>c_M=c_P</math>.
 
  
For an ideal gas, <math>c_P=c_V+R</math>.
+
where
For an incompressible substance, <math>c_P=c_V</math>.
+
<math>\Delta Q</math> is the change in heat, <math>n</math> is the number of moles of substance, <math>c_M</math> is the molar heat capacity, and
 +
<math>\Delta T</math> is the change in temperature.
 +
 
 +
At constant volume, <math>c_M=c_V</math>. At constant pressure, <math>c_M=c_P</math>.
 +
 
 +
For an ideal gas, <math>c_P=c_V+R</math> where <math>R=</math> the ideal gas constant. For an incompressible substance, <math>c_P=c_V</math>.
  
 
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>.
 
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>.
 +
 +
== See Also ==
 +
*An excellent derivation of the last equation can be found [https://www.animations.physics.unsw.edu.au/jw/Adiabatic-expansion-compression.htm here].
 +
* [[Heat]]
 +
* [[Thermodynamics]]
 +
 +
 +
[[Category: Physics]]
 +
{{stub}}

Latest revision as of 11:02, 1 August 2020

The molar heat capacity is the amount of energy required to change the temperature of an amount of substance by a certain amount per moles of the substance and change in temperature.

Adding heat to a substance changes its temperature in accordance to \[\Delta Q=nc_M\Delta T,\]

where $\Delta Q$ is the change in heat, $n$ is the number of moles of substance, $c_M$ is the molar heat capacity, and $\Delta T$ is the 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 $\gamma=\frac{c_V+R}{c_V}$.

See Also

This article is a stub. Help us out by expanding it.

Invalid username
Login to AoPS