Entropy and Second Law of Thermodynamics

What is the entropy change (in ${\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}$ ) when one mole of ice is converted into water at  $0°\mathrm{C}$? (The enthalpy change for the conversion of ice to liquid water  $6.0\hspace{0.17em}\mathrm{kJ}\hspace{0.17em}{\mathrm{mol}}^{-1}\mathrm{\hspace{0.17em}}\mathrm{at}\mathrm{\hspace{0.17em}}0°\mathrm{C}$)

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. $\left(\mathrm{R}=2 \mathrm{cal}/\mathrm{mol} \mathrm{K}\right)$    

One mole of an ideal gas at $350 \mathrm{K}$ is in a $2.0 \mathrm{L}$ vessel of thermally conducting walls, which are in contact with the surroundings. It undergoes isothermal reversible expansion from $2.0 \mathrm{L}$ to $3.0 \mathrm{L}$ against a constant pressure of $4 \mathrm{atm}$. The change in entropy of the surroundings $(∆\mathrm{S})$ is _____ $\mathrm{J} {\mathrm{K}}^{–1}$ (Nearest integer)

Given: $R=8.314 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$.

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R

Assertion A: In the Ellingham diagram, a sharp change in slope of the line is observed from $\mathrm{Mg}\to \mathrm{MgO}$ at $~{1120}^{\mathrm{o}}\mathrm{C}$

Reason R: There is a large change of entropy associated with the change of state

In the light of the above statements, choose the correct answer from the options given below

$30.4 \mathrm{kJ}$ of heat is required to melt one mole of sodium chloride and the entropy change at the melting point is $28.4 \mathrm{J} {\mathrm{K}}^{–1} {\mathrm{mol}}^{–1}$ at $1 \mathrm{atm}$. The melting point of sodium chloride is _______ $\mathrm{K}$ (Nearest Integer value)

Why entropy increases from solid to liquid?

One mole of ice is converted into water at $0°\mathrm{C}$. The enthalpy change for the conversion of ice into liquid water is $6.0 \mathrm{kJ} {\mathrm{mol}}^{-1}$ at $0°\mathrm{C}$. Correct among the following is

In which of the following reactions, standard reaction entropy change ($∆\mathrm{S}°$) is positive and standard Gibb's energy change ($∆\mathrm{G}°$) decreases sharply with increasing temperature?

For the reaction,
${\mathrm{CaCO}}_3\left(\mathrm{s}\right) \to \mathrm{CaO}\left(\mathrm{s}\right) + {\mathrm{CO}}_2\left(\mathrm{g}\right),$
the correct option is

Third law of thermodynamics deals with

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

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 

Calculate the melting point of $\mathrm{KCl}\left(\mathrm{s}\right)$ from the data, ${∆}_{\mathrm{fus}}\mathrm{H}\left(\mathrm{KCl}\right)=7.25 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and ${∆}_{\mathrm{fus}}\mathrm{S}\left(\mathrm{KCl}\right)=7 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$.

What is the sign of $∆\mathrm{S}$ for the following reaction?

${\mathrm{CaCO}}_3\left(\mathrm{s}\right)\stackrel{ }{\to }\mathrm{CaO}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$

What does entropy measure?

Write any two applications of 'second law of thermodynamics'.