91Ó°ÊÓ

$P_{\text{initial}}<P_{\text{final}}$

$V_{\text{initial}}=V_{\text{final}}$

formula used:

$Q=\mathrm{Δ}U-W$

if$W=0→Q=\mathrm{Δ}U$

$\mathrm{Δ}U=m{C}_v\mathrm{Δ}T$

Heat transfer into or out of the system does not change the P?V work, but simply changes the internal energy (temperature) of the system, because the volume remains constant.

The pressure-volume work is zero since the process is isochoric, $V=0$. The internal energy may be computed using the ideal gas model by:

$\mathrm{Δ}U=m{C}_v\mathrm{Δ}T$

The property is referred to as "specific heat" (or heat capacity) at a constant volume because it relates the temperature change of a system to the amount of energy added by heat transfer under particular unique conditions (constant volume).

The first law of thermodynamics states that there is no work done by or on the system.

$U=?Q.$

To make the graph, you must first understand the principles and procedure.