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

`$\Delta S = -10.95 \ (J)/(K)$`

Step-by-step 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,

`$\Delta S = c_V\ln \left((T_2)/(T_1)\right) + n R \ln \left((V_2)/(V_1)\right)$`

For isothermal compression temperature constant,

`$\Delta S = n R \ln \left((V_2)/(V_1)\right)$`

`$\Delta S = 0.720 * 8.314 * \ln \left((3.90)/(24.32)\right)$`

`$\Delta S = -10.95 \ JK^(-1)$`

`$\Delta S = -10.95 \ (J)/(K)$`