SL: Entropy of a Irreversible Isothermal Expansion

Entropy of a Irreversible Isothermal Expansion

Example:

The same piston-cylinder assembly is now loaded with a single weight to yield the same initial pressure of 2 bar. The weight is removed all at once. The initial and final P,V,T are the same as the previous example. Represent this on a PV and PT diagram. Find the total heat transfer, and the entropy change of the system, the surroundings, and the universe.

Note:

In order to calculate $\Delta S_{sys}$ we must always use the reversible process, so even for the irreversible process, we get
$\Delta S_{sys} = 5.76 J/K$

$\Delta S_{surr} = \int_{initial}^{final} \frac{\delta Q_{surr}}{T}$

Recall:

Our first law analysis of this problem yields:

$Q_{sys}=-W = -(-\int P_E dV) = nP_2 \left (\hat V_2 - \hat V_1 \right )$

$\Delta S_{surr} = -\int_{initial}^{final} \frac{nP_2 \left (\hat V_2 - \hat V_1 \right )}{T}$

$\Delta S_{surr} = -\frac{nP_2}{T_1} \left (\hat V_2 - \hat V_1 \right ) = -\frac{(1 mol)(1 bar)}{962 K}\left (0.08m^3/mol - 0.04m^3/mol \right ) = -4.16 J/K$

$\Delta S_{univ} = \Delta S_{sys} + \Delta S_{surr}$

$\Delta S_{univ} = 5.75 J/K - 4.16 J/K = 1.59 J/K$

Outcome:

Identify, formulate, and solve simple engineering problems (such as expansion/compression and power cycles)