Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

The Haber’s process for the formation of ${\mathrm{NH}}_3$ at $298 \mathrm{K}$ is ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3;\mathrm{\hspace{0.17em}}\mathrm{\Delta H}=-46.0\mathrm{KJ}$. Which of the following is the correct statement?

Consider the curve between $\ln \mathrm{K}$ and $1/\mathrm{T}$. Which plot will be correct for exothermic reaction?

The ionisation constant of ${\mathrm{NH}}_4^{+}$ in water is $5.6\times {10}^{-10}$ at $25°\mathrm{C}$. The rate constant for the reaction of ${\mathrm{NH}}_4^{+}$ and ${\mathrm{OH}}^{-}$ to form ${\mathrm{NH}}_3$ and ${\mathrm{H}}_2\mathrm{O}$ at $25°\mathrm{C}$ is $3.4\times {10}^{10} \mathrm{L} {\mathrm{mol}}^{-1}{\sec }^{-1}$. If dissociation constant of water at $25°\mathrm{C}$ is $1.8\times {10}^{-16}$. If ${\mathrm{K}}_{\mathrm{w}}$ of water at $60°\mathrm{C}$ is $9.5\times {10}^{-14},$ then the heat of neutralisation is:

The change in standard Gibbs energy for a reaction at equilibrium, $eg . \mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g),$ on addition of an inert gas at constant pressure and then at constant volume respectively are :

$5$ moles of $N_2{O}_4$ taken in a one litre flask dissociates to$20\%$ extent to reach equilibrium. What is $\Delta G°$ of the reaction ?

$\underset{\left(g\right)}{N_2{O}_4}\stackrel{}{\rightleftharpoons }\underset{\left(g\right)}{2N{O}_2}$

$MC{O}_3 \left(s\right)\rightleftharpoons MO \left(s\right)+C{O}_2 \left(g\right)$ the equilibrium pressure of $C{O}_2$ at ${127}^{o}C$ and ${147}^{o}C$ are $0.14$ and $0.35$ bar respectively. Then :

Consider the reaction :

$A\rightleftharpoons B \Delta H_f^{\circ } kJ S^{\circ }J{K}^{-1}$

$A -24.27 246.4$

$B -25.44 252.3$

Then the composition of the equilibrium mixture at ${25}^{o}C$ is

The equilibrium constant for a reaction is 10. $\mathrm{\Delta }{G}^o$ will be $\left(R=8\mathrm{J}{\mathrm{K}}^{-1}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1},T=300\mathrm{K}\right)$

What are the values of $∆{\mathrm{G}}^{\mathrm{o}}$ and the equilibrium constant for the formation of $\mathrm{N}{\mathrm{O}}_2$ from $\mathrm{NO}$ and ${\mathrm{O}}_2$ at $298$ K. Given $\log \left(1.365\times {10}^6\right)=6.14$

$\mathrm{N}\mathrm{O}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\to \mathrm{N}{\mathrm{O}}_2\left(\mathrm{g}\right)$ where $∆{\mathrm{G}}_{\mathrm{f}}^{\mathrm{o}}=52.0\mathrm{ }\mathrm{k}\mathrm{J}/\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }$

$∆{\mathrm{G}}_{\mathrm{r}}^{\mathrm{o}}\left(\mathrm{NO}\right)=87.0\mathrm{ }\mathrm{k}\mathrm{J}/\mathrm{m}\mathrm{o}\mathrm{l}$

$∆{\mathrm{G}}_{\mathrm{r}}^{\mathrm{o}}\left({\mathrm{O}}_2\right)=0\mathrm{ }\mathrm{k}\mathrm{J}/\mathrm{m}\mathrm{o}\mathrm{l}$

Calculate ${\mathrm{K}}_{\mathrm{p}}$ for the reaction

$\frac{3}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{O}}_3\left(\mathrm{g}\right)$ at 298 K $.\mathrm{D}{\mathrm{G}}^{\mathrm{o}}$ for the reaction is $163.43\mathrm{ }\mathrm{k}\mathrm{J}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ is

Which of the following statements is correct for a reversible process in a state of equilibrium?

A schematic plot of ${\mathrm{lnK}}_{\mathrm{eq}}$ versus $\frac{1}{\mathrm{T}}$ for a reaction is shown below:

The reaction must be:

The value of  ${\mathrm{logK}}_{\mathrm{c}}$ for a reaction  $\mathrm{A}\leftrightharpoons \mathrm{B}$ is?

(Given, ${∆}_{\mathrm{r}}\mathrm{H}° 298\mathrm{ }\mathrm{K}=-54.07\mathrm{ }\mathrm{kJ}\mathrm{ }{\mathrm{mol}}^{-1},$$\mathrm{ }{∆}_{\mathrm{r}}\mathrm{S}° 298\mathrm{ }\mathrm{K}=10\mathrm{ }{\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}\mathrm{ }$and $\mathrm{R}=8.314\mathrm{ }{\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}\mathrm{ }2.303\times 8.314\times 298=5705)$

The standard entropies of ${\mathrm{X}}_2, {\mathrm{Y}}_2$ and ${\mathrm{XY}}_3$ are $60, 40$ and $50 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$, respectively. For the reaction $\frac{1}{2}{\text{X}}_2+\frac{3}{2}{\text{Y}}_2\rightleftharpoons {\text{XY}}_3, \Delta \text{H}=-30\text{ kJ}$, to be at the equilibrium, the temperature should be

Which is/are correct ?

For the equilibrium at $298 \mathrm{K},$ ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$; ${\mathrm{G}}_{{\mathrm{N}}_2{\mathrm{O}}_4}^{\mathrm{o}}=100 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and ${\mathrm{G}}_{{\mathrm{NO}}_2}^{\mathrm{o}}=50 \mathrm{kJ} {\mathrm{mol}}^{-1}$. $5$ moles of ${\mathrm{N}}_2{\mathrm{O}}_4$ and $2$ moles of ${\mathrm{NO}}_2$ are taken initially in a one-litre container, then, which statements are correct?

The correct statement regarding a reversible system is (are):

The equilibrium constant of the following reaction in equilibrium at $27^{\circ }\text{C}$ 
$\text{A}+\text{B}\rightleftharpoons \text{C}+\text{D}$  is 10
Which of the following statements are correct?

Which of the following statements is true? 

For a given reaction, $\mathrm{K}=1·7\times {10}^7$ at $25^{\circ }\text{C}$.
${\text{Ag}}^{+}\left(\text{aq}\right)+2{\text{NH}}_3\left(\text{aq}\right)\rightleftharpoons {\left[\text{Ag}{\left({\text{NH}}_3\right)}_2\right]}^{+}$
What is the value of $\Delta {\text{G}}^{\circ }$in $\mathrm{kJ}$?