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[A]$\Delta G=RT{{\log }_{e}}{{K}_{p}}$

[B]$-\Delta G=RT{{\log }_{e}}{{K}_{p}}$

[C]$\Delta G=R{{T}^{2}}\ln {{K}_{p}}$

[D] None of these

Answer

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We know that, we can write the Gibbs free energy as a function of temperature and pressure, which gives us the relation-

\[\Delta G=\Delta {{G}^{\circ }}+nRT\ln P\]

Where, $\Delta G$ is the change in Gibbs free energy and $\Delta {{G}^{\circ }}$ is the change in Gibbs free energy in standard conditions.

R is the universal gas constant, R= 8.314 J/mol.K

T is the temperature and P is the pressure.

As we know that in thermodynamics, the Van't Hoff equation gives us a relation between the equilibrium constant and the change in Gibbs free energy of a chemical reaction where change is in standard conditions.

Let us take a system at equilibrium like-

\[aA+bB\rightleftharpoons cC+dD\]

The equilibrium constant for the above reaction will be ${{K}_{eq}}=\dfrac{{{\left[ C \right]}^{c}}{{\left[ D \right]}^{d}}}{{{\left[ A \right]}^{a}}{{\left[ B \right]}^{b}}}$

The Gibbs free energy of the component ‘A’ will be $a{{G}_{A}}=a{{G}_{A}}^{\circ }+aRT\ln {{P}_{A}}$ (by putting ‘a’ in the Gibbs free energy equation)

Similarly, we can write that Gibbs free energy of the component ‘B’, ‘C’ and ‘D’ will be-

$\begin{align}

& b{{G}_{B}}=b{{G}_{B}}^{\circ }+bRT\ln {{P}_{B}} \\

& c{{G}_{C}}=c{{G}_{C}}^{\circ }+cRT\ln {{P}_{C}} \\

& d{{G}_{D}}=d{{G}_{D}}^{\circ }+dRT\ln {{P}_{D}} \\

\end{align}$

As, the total change in Gibbs free energy can be written as the difference of change in free energy of the product and the reactant, which we can write as-

$\Delta G=\sum{{{G}_{P}}-\sum{{{G}_{R}}}}$

We have calculated the free energy of the reactant and the product before, so putting those values in the above equation and rearranging the equation, we will get-

\[\Delta G=\left\{ c{{G}_{C}}^{\circ }+d{{G}_{D}}^{\circ } \right\}-\left\{ a{{G}_{A}}^{\circ }+b{{G}_{B}}^{\circ } \right\}+\left\{ RT\ln \left[ \dfrac{{{P}_{C}}^{c}\times {{P}_{D}}^{d}}{{{P}_{A}}^{a}\times {{P}_{B}}^{b}} \right] \right\}\]

We can write,\[\Delta {{G}^{\circ }}=\left\{ c{{G}_{C}}^{\circ }+d{{G}_{D}}^{\circ } \right\}-\left\{ a{{G}_{A}}^{\circ }+b{{G}_{B}}^{\circ } \right\}\]as it is the change in free energy in standard condition. Therefore, equation becomes

\[\Delta G=\Delta {{G}^{\circ }}+\left\{ RT\ln \left[ \dfrac{{{P}_{C}}^{c}\times {{P}_{D}}^{d}}{{{P}_{A}}^{a}\times {{P}_{B}}^{b}} \right] \right\}\]

Now at equilibrium,$\Delta G=0,\left[ \left[ \dfrac{{{P}_{C}}^{c}\times {{P}_{D}}^{d}}{{{P}_{A}}^{a}\times {{P}_{B}}^{b}} \right] \right]={{K}_{p}}$

So, we can write the equation as-

\[\begin{align}

& 0=\Delta {{G}^{\circ }}+RT\ln {{K}_{p}} \\

& or,\Delta {{G}^{\circ }}=-RT\ln {{K}_{p}} \\

\end{align}\]

This is the Van’t Hoff isotherm equation which gives us a relation between the standard Gibbs free energy and the equilibrium constant.

The Van’t Hoff isotherm equation is used for estimating the equilibrium shift during a chemical reaction. We can also derive the Van’t Hoff isotherm equation using the Gibbs-Helmholtz equation which gives a relation between the change in free energy with respect to the changing temperature.