Exploration 20.6: Specific Heat at Constant Pressure and
check to have integral calculated.
Please wait for the animation to
There is a time delay—since the system must be
in equilibrium—before the change of state occurs.
In this animation N = nR (i.e., kB = 1). This, then, gives
the ideal gas law as PV = NT.
For an ideal monatomic gas, the change in internal energy depends only on
temperature, ΔU = (3/2)nRΔT = (3/2)NΔT
Calculate the change in internal energy for the three cases.
What is the work done in each case? As a reminder, W = ∫
P dV, and pressure can (and does in many instances) depend on volume.
Calculate the work done in each case using the following two methods, then
compare your answers.
Graphically: To find the work done is to determine the area under the
curve ("area" of the red region on the graph). After estimating the area by
counting the grid blocks, click the checkbox above to show a calculation of the area
(by numerical integration) on the simulation. Explain any significant
differences between your estimation and the numerical integration.
Analytic solution (a little bit of calculus required): When heat is added
at constant pressure (isobaric process), then P, pressure, in the above equation for work is simply a
constant of integration. When heat is added at a constant volume
the work done is zero. Why? When heat is added at a constant temperature
use the ideal gas law (PV = NT) and write the pressure as a function of volume:
NT/V (where N and T are constant) and then you can integrate (the answer involves a natural logarithm).
Using the first law of thermodynamics, Q = W + ΔU,
calculate the heat input and show that it is the same for all three cases.
The specific heat capacity of a material is a measure of the quantity of
heat needed to raise a gram (or given quantity) of a material 1oC.
For a gas, it requires a different amount of heat to raise the same amount of
gas to the same temperature depending on the circumstances under which the heat
is added. If the same amount of heat is added, the final temperatures of
the constant pressure and constant volume expansions are quite different (and,
for a constant temperature, heat is added but the temperature does not
In which case does the heat input raise the temperature the
So, if the specific heat capacity of an ideal gas is to have any meaning at all,
it must be defined in terms of the process: specific heat at a constant volume
or specific heat at a constant pressure.
Go back to your calculation of heat in (c). Calculate the constant of
proportionality between heat input and the change in temperature for the constant
volume and constant pressure cases: Q = (Constant)NΔT.
What is the constant in each case? Why is the constant for an
expansion at constant pressure greater? (Hint: Think about whether the
heat is used only to change temperature or to change temperature and do work.)
Generally, we write the heat capacity as a molar heat capacity (where n is
the number of moles) and find that for constant pressure Q = CPnΔT and CP = (5/2)R, and for constant volume Q = CVnΔT and CV = (3/2)R.
We began this discussion by
noting that for an ideal monatomic gas, the average internal energy is (3/2)T.
This comes from kinetic theory and the equiparititon of energy, where the 3 comes from 3 degrees of freedom. For a diatomic gas, the
average internal energy is (5/2)T because there are two more degrees of
How are the heat capacity at a constant
pressure and heat capacity at a constant volume different for a diatomic gas?
When you get
a good-looking graph, right-click on it to clone the graph and resize it for a