Spontaneity

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

For a spontaneous process,
 

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

Matching Type Question

The standard entropy change accompanying the cell reaction will be

Enthalpy change for the process,
${\mathrm{H}}_2\mathrm{O}\left(\mathrm{i}\mathrm{c}\mathrm{e}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{O}\left(\mathrm{w}\mathrm{a}\mathrm{t}\mathrm{e}\mathrm{r}\right)$ is $6.01\mathrm{ }\mathrm{k}\mathrm{J}\mathrm{ }\mathrm{m}\mathrm{o}{{\mathrm{l}}^{-}}^1$ ,
the entropy change of $1$ mole of ice at its melting point will be

Calculate$∆{\mathrm{S}}_{\mathrm{total}}$  hence show whether the following reaction is spontaneous at $25°\mathrm{C}$$\mathrm{Hg} \left(s\right) + {\mathrm{O}}_2 \left(\mathrm{g}\right) \to \mathrm{Hg}\left(\mathrm{l}\right) + {\mathrm{SO}}_2 \left(\mathrm{g}\right) ∆\mathrm{H}° =-238.6 \mathrm{kJ} \mathrm{and} ∆\mathrm{S}° = +36.7 \mathrm{J} {\mathrm{K}}^{-1}$

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

Which of the following processes is nonspontaneous?

For the conversion of liquid to solid below the melting point of solid

For the process, ${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)⟶{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\text{ at }100°\mathrm{C}. ∆\mathrm{S}$ is

Which member of the pair has larger entropy and why? $\mathrm{Na} \left(\mathrm{s}\right)$ or $\mathrm{NaCl} \left(\mathrm{s}\right)$.

Which member of the pair has larger entropy and why? $\mathrm{Xe} \left(\mathrm{g}\right)$ or $\mathrm{Kr} \left(\mathrm{g}\right)$.

Which member of the pair has larger entropy and why? $\mathrm{NO} \left(\mathrm{g}\right)$ or ${\mathrm{N}}_2{\mathrm{O}}_4 \left(\mathrm{g}\right)$.

Which member of the pair has larger entropy and why? ${\mathrm{CH}}_3\mathrm{OH} \left(\mathrm{l}\right)$ or ${\mathrm{C}}_2{\mathrm{H}}_5{\mathrm{OC}}_2{\mathrm{H}}_5 \left(\mathrm{l}\right)$.