Gibbs Free Energy or Gibbs Function

Given, $\mathrm{\Delta G}°=-{\mathrm{nFE}}_{\text{cell }}°$ and $\mathrm{\Delta G}°=-\mathrm{RT} \ln \mathrm{k}$. The value of $\mathrm{n}=\frac{\mathrm{F}}{\mathrm{RT}}$ will be given by the slope of which line in the figure

Which one of the following is correct?

A plot of $\ln \mathrm{K}$ against $\frac{1}{\mathrm{T}}$ (abscissa) is expected to be a straight line with intercept on ordinate axis equal to

Which of the following conditions will apply to the conversion of ice into water?

For the precipitation reaction of ${\mathrm{Ag}}^{+}$ ions with $\mathrm{NaCl}$, which of the following statements is correct?

The densities of graphite and diamond at $298 \mathrm{K}$ are $2.25$ and $3.31 \mathrm{g} {\mathrm{cm}}^{-3}$, respectively. If the standard free energy difference $\left(\mathrm{\Delta G}°\right)$ is equal to $1895 \mathrm{J} {\mathrm{mol}}^{-1}$, the pressure at which graphite will be transformed into diamond at $298 \mathrm{K}$ is

$$\begin{gathered} {\mathrm{PbO}}_2\to \mathrm{PbO}; {\mathrm{\Delta G}}_{298 \mathrm{K}}<0 \\ {\mathrm{SnO}}_2\to \mathrm{SnO}; {\mathrm{\Delta G}}_{298 \mathrm{K}}>0 \end{gathered}$$

The most probable oxidation state of $\mathrm{Pb}$ and $\mathrm{Sn}$ will be

The factor of $\mathrm{\Delta G}$ values is important in metallurgy. The $\mathrm{\Delta G}$ values for the following reactions at $800°\mathrm{C}$ are given as:

${\mathrm{S}}_2 \left(\mathrm{s}\right)+2{\mathrm{O}}_2 \left(\mathrm{g}\right)⟶2{\mathrm{SO}}_2 \left(\mathrm{g}\right); \mathrm{\Delta G}=-544 \mathrm{kJ}$
$2\mathrm{Zn} \left(\mathrm{s}\right)+{\mathrm{S}}_2 \left(\mathrm{s}\right)⟶2\mathrm{ZnS} \left(\mathrm{s}\right); \mathrm{\Delta G}=-293 \mathrm{kJ}$
$2\mathrm{Zn} \left(\mathrm{s}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)⟶2\mathrm{ZnO} \left(\mathrm{s}\right); \mathrm{\Delta G}=-480 \mathrm{kJ}$

$\mathrm{\Delta G}$ for the below reaction will be

$2\mathrm{ZnS} \left(\mathrm{s}\right)+3{\mathrm{O}}_2 \left(\mathrm{g}\right)⟶2\mathrm{ZnO} \left(\mathrm{s}\right)+2{\mathrm{SO}}_2 \left(\mathrm{g}\right)$

Match List $\mathrm{I}$ (Equations) with List $\mathrm{II}$ (Types of process) and select the correct option.

What is the free energy change for the conversion of $1$ mole of water into steam at $373.2 \mathrm{K}$. The heat of vaporization $\left(∆{\mathrm{H}}_{\mathrm{v}}\right)$ of water at $373.2 \mathrm{K}$ is $9.1 \mathrm{kcal} {\mathrm{mol}}^{-1}$. The entropy change is $25.5 \mathrm{cal} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}$.

In an irreversible process taking place at constant $\mathrm{T}$ and $\mathrm{P}$ and in which only the pressure-volume work is being done, the change in Gibbs free energy ($\mathrm{dG}$) and the change in entropy ($\mathrm{dS}$) satisfy the criteria

A certain reaction is non-spontaneous at $298 \mathrm{K}$. The entropy change during the reaction is $121 \mathrm{J} {\mathrm{K}}^{-1}$. Is the reaction endothermic or exothermic? The minimum value of $\mathrm{\Delta H}$ for the reaction is

What is the free energy change $\left(\mathrm{\Delta G}\right)$ when $1.0 \mathrm{mol}$ of water at $100°\mathrm{C}$ and $1 \mathrm{atm}$ pressure is converted into steam at $100°\mathrm{C}$ and $1 \mathrm{atm}$ pressure?

Gibbs free energy for the reaction at equilibrium is

A spontaneous reaction is impossible if

Identify the correct statement for the change of Gibbs energy for a system (${\mathrm{\Delta G}}_{\mathrm{system} }$) at constant temperature and pressure.

The enthalpy and entropy change for the reaction ${\mathrm{Br}}_2 \left(\mathrm{I}\right)+{\mathrm{Cl}}_2 \left(\mathrm{g}\right)\to 2\mathrm{BrCl} \left(\mathrm{g}\right)$ are $30 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and $105 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$, respectively. The temperature at which the reaction will be in equilibrium is

Which of the following pairs of chemical reactions is certain to result in a spontaneous reaction?

The standard enthalpy and standard entropy changes for the oxidation of ammonia at $298 \mathrm{K}$ are $-382.64 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and $-145.6 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$, respectively. The standard Gibbs energy change for the same reaction at $298 \mathrm{K}$ is

Standard Gibbs free energy change for isomerisation reaction cis-$2$ pentene $\rightleftharpoons$trans-$2$ pentene is $-3.67 \mathrm{kJ}/\mathrm{mol}$ at $400 \mathrm{K}$. If more trans-$2$ pentene is added to the reaction vessel,