Question

. Calculate the entropy change associated with the isothermal compression of 0.720 mol of an ideal gas from 24.32 L to 3.90 L.

Answer 1

Answer:

$\Delta S = -10.95 \ \frac{J}{K}$

Explanation:

Given :

Number of mole, n = 0.720 mol

Initial volume, $V_1$ = 24. 32 L

Final volume, $V_2$ = 3.90 L

We know entropy change,

$\Delta S = c_V\ln \left(\frac{T_2}{T_1}\right) + n R \ln \left(\frac{V_2}{V_1}\right)$

For isothermal compression temperature constant,

$\Delta S = n R \ln \left(\frac{V_2}{V_1}\right)$

$\Delta S = 0.720 \times 8.314 \times \ln \left(\frac{3.90}{24.32}\right)$

$\Delta S = -10.95 \ JK^{-1}$

$\Delta S = -10.95 \ \frac{J}{K}$