Entropy and Second Law of Thermodynamics

Unit of entropy is:

$2 \mathrm{mol}$ of an ideal gas at  $27°\mathrm{C}$ temperature is expanded reversibly from $2 \mathrm{L}$ to $20 \mathrm{L}$. Find the entropy change. $\left(\mathrm{R}=2 \mathrm{cal}/\mathrm{mol} \mathrm{K}\right)$    

The adsorption of a gas at the boiling point of the gas follows the isotherm shown in the figure. Identify the correct thermodynamic properties at point $C.$

A heat engine absorbs heat ${\mathrm{Q}}_1$ at temperature ${\mathrm{T}}_1$ and heat ${\mathrm{Q}}_2$ at temperature ${\mathrm{T}}_2$. Work done by the engine is $\left({\mathrm{Q}}_1+{\mathrm{Q}}_2\right) \mathrm{J}$. This data

For which of the following processes, $∆\mathrm{S}$ is negative?

The molar heat capacity (${\mathrm{C}}_{\mathrm{p}}$) of ${\mathrm{CD}}_2\mathrm{O}$ is $10 \mathrm{cal}$ at $1000\mathrm{K}$. The change in entropy associated with cooling of $32\mathrm{g}$ of ${\mathrm{CD}}_2\mathrm{O}$ vapour from$1000\mathrm{K}-100\mathrm{K}$ at constant pressure will be : ($\mathrm{D}$ = deuterium, Atomic mass = $2$) 

The enthalpy of vaporization of water at $100°\mathrm{C}$ is $40.63 {\mathrm{kJmol}}^{-1}$. Its entropy of vaporization would be

The $\mathrm{SI}$ unit of $∆\mathrm{S}$ is 

What does entropy measure?

A container is divided into two compartments by a removable partition as shown below:

In the first compartment, ${\mathrm{n}}_1$ moles of ideal gas He is present in a volume ${\mathrm{V}}_1.$ In the second compartment, ${\mathrm{n}}_2$ moles of ideal gas $\mathrm{Ne}$ is present in a volume ${\mathrm{V}}_2.$ The temperature and pressure in both the compartments are $\mathrm{T}$ and $\mathrm{P},$ respectively. Assuming $\mathrm{R}$ is the gas constant, the total change in entropy upon removing the partition when the gases mix irreversibly is:

The change in entropy at equilibrium is 

The enthalpy of vaporization of water at $100°\mathrm{C}$ is $40.63 {\mathrm{kJmol}}^{-1}$. Its entropy of vaporization would be

$\mathrm{\Delta S}$ will be highest for

Among the following processes, for which process the change in entropy $\left(\mathrm{\Delta S}\right)$ is negative?

$2$ mole of an ideal gas at $27°\mathrm{C}$ expands reversibly from $2$ litre to $20$ litre. The entropy change is: $\left(\mathrm{R}=2 \mathrm{cal} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}\right)$

A sample of an ideal gas is expanded to twice its original volume of 1 m³ in a reversible process for which $\text{α}={\text{5 atm m}}^{-6}$  and ${\text{C}}_{\text{Vm}}={\text{20 J K}}^{-1}{m}^{-1}$ at constant volume.

The entropy change during the process may be (polytropic process given by function P = αv²)

The standard entropy change accompanying the cell reaction will be